Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > 2.1.4 Acids + 2.1.5 Redox > Flashcards

2.1.4 Acids + 2.1.5 Redox Flashcards

1
Q

what is the formula for ethanoic acid?

A

CH3COOH

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

what is the formula for sodium carbonate?

A

Na2CO3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what is the formula for phosphoric acid?

A

H3PO4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what is the definition of an acid?

A

in water an acid releases hydrogen ions into solutions (a proton donor)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

what is the definition of a hydrogen ion?

A

a hydrogen ion has no electrons in its outer shell , it is known as a proton

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

what is the definition of a strong acid?

A

a strong acid releases all of its hydrogen ions in the solution and is completely dissociated / ionised

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

what is the definition of a weak acid?

A

a weak acid only releases a small number of its hydrogen ions in solution and partially dissociates / ionises

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

when a strong acid dissociates is it a reversible reaction?

A

NO

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

when a weak acid dissociates is it a reversible reaction?

A

YES

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

what is the definition of a base?

A

a compound that neutralises an acid, by accepting a hydrogen ion, to form a salt (proton acceptor)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

what are bases usually?

A

metal oxides or ammonia

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

how do bases form dative covalent bonds?

A

bases donate 2 electrons to the hydrogen ion to form a dative covalent bond

bases can either have a lone pair or negative charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

what is the definition of an alkali?

A

an alkali is a soluble base that releases hydroxide ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

give examples of common alkalis used

A

hydroxides

NaOH

KOH

Ca(OH)2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

what is the definition of a salt?

A

a salt is the product of a reaction in which H+ ions from the acid are replaced by the metal or ammonium ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

what does a metal + acid make?

A

salt + hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

what does a metal oxide (base) + acid make?

A

salt + water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

what does a metal hydroxide + acid make?

A

salt + water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

what does a metal carbonate + acid make?

A

salt + carbon dioxide + water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

what does ammonia + acid make?

A

ammonium salt

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

what is the method for making a standard solution?

A

1 - weigh out the mass of the solid using weigh by difference to 2 decimal places

2 - place the solid into a beaker

3 - add 10cm3 of distilled water to the beaker

4 - stir the solution to dissolve the solid

5 - transfer the solution to a 250cm3 volumetric flask

6 - rinse the equipment into the volumetric flask

7 - make up the solution to the 250cm3 line with distilled water, using a pipette, the bottom of the meniscus should be on the line

8 - put on the lid and invert several times to mix

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

what are concordant results?

A

results within 0.1cm3 of each other

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

what results must you only use in the titration calculation?

A

concordant results

do not use rough

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

what is the equation for the titration calculation?

A

moles = conc x volume
———————-
1000

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

what are the steps for the titration calculation?

A

1 - moles

2 - ratio

3 - apply to question

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

what is the method for a titration?

A

1 - rinse all glass wear with distilled water and the solution that will be used

2 - measure 25cm3 of the standard solution with a pipette and filler and put in conical flask

3 - add 3 drops of indicator

4 - place on white tile

5 - using a funnel fill the biurette with acid, to the zero mark with the bottom of the meniscus on this line

6 - complete a rough titration, looking for the end point while swirling the conical flask

7 - repeat the experiment adding the acid drop by drop to reach the endpoint

8 - rinse conical flask between titrations with distilled water

9 - record out titres into a table

10 - calculate the mean titre using concordant results

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

what is uncertainty of a piece of equipment?

A

half the smallest possible unit you can make

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

what is the equation for percentage uncertainty?

A

uncertainty of equipment
————————————- X100
size of measurement

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

what do you need to take into account when working out the percentage uncertainty?

A

how many times you have read off that piece of equipment to get one answer

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

what are steps for the harder titration calculation questions?

A

1 - read question and draw diagram to understand what is in what equipment

2 - moles

3 - ratio

4 - often moles in volumetric flask

5 - answer question

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

what is a volumetric flask?

A

a type of laboratory flask, calibrated to contain a precise volume at a particular temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

what are volumetric flasks used for?

A

precise dilutions and preparation of standard solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

what is the equation for new concentration?

A

original vol
—————- X original concentration
new vol

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

what is the definition of an oxidation number?

A

a measure of the number of electrons that an atom uses to bond with an atom of another element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

what is the oxidation number of a neutral atom?

A

zero

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

what is the oxidation number of a monatomic atom?

A

the same as the charge on the ion e.g. O2- = -2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

what is the sum of all oxidation numbers in a polyatomic ion?

A

equal to the charge on the ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

what is the sum of all oxidation numbers in a neutral compound?

A

zero

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

what is usually the oxidation state of hydrogen?

A

+1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

what is the oxidation state of hydrogen when it is part of a binary metal hydride?

A

-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

what does fluorine always have an oxidation number of in a compound?

A

-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

what is the oxidation number of oxygen usually in a compound?

A

-2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

what is the oxidation number of oxygen if it is in a peroxide compound?

A

-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

when does oxygen have an oxidation number of +1?

A

when bonded to fluorine

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
45
Q

in what group can oxidation numbers vary?

A

transition metals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
46
Q

what usually are chlorine, bromine and iodine’s oxidation numbers?

A

-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
47
Q

when do halogens not have oxidation number of -1?

A

when in a compound with oxygen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
48
Q

what do we do when a compound needs a systematic name?

A

write the oxidation number in Roman numerals in brackets after the elements name in a compound

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
49
Q

what is the definition for redox reaction?

A

a reaction involving oxidation and reduction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
50
Q

what does OIL RIG stand for?

A

oxidation is loss of electrons

reduction is gaining of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
51
Q

what are the two different types of ways of working out a redox reaction?

A

electron transfer

oxidation numbers

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
52
Q

what is the rule when working out what is oxidised and reduced in a reaction using oxidation numbers?

A

if the oxidation number increases it is oxidation

if the oxidation number decreases it is reduction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
53
Q

what do you have to write in your answer when working out what is oxidised and reduced in a reaction?

A

state the element and how the oxidation number has changed and what it has changed from

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
54
Q

what is the reaction called if the same element is oxidised and reduced?

A

disproportination

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
55
Q

What is the ideal gas equation?

A

PV = nRT

P = Pressure, V = Volume, n = moles, R = 8.31 JK-1mol-1, T = Temperature in Kelvin

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
56
Q

What are the units for Pressure (P) in the ideal gas equation?

A

Pa

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
57
Q

What are the units for Volume (V) in the ideal gas equation?

A

m³

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
58
Q

What are the units for Temperature (T) in the ideal gas equation?

A

K

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
59
Q

What is the value of R in the ideal gas equation?

A

8.31 JK-1mol-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
60
Q

How do you convert temperature from Celsius to Kelvin?

A

Add 273

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
61
Q

Convert 20°C to Kelvin.

A

293 K

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
62
Q

Convert 500 cm³ to m³.

A

0.0005 m³

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
63
Q

Calculate the moles of gas using the ideal gas equation.

A

moles = PV/RT

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
64
Q

What is the mass of Cl gas given a pressure of 100 kPa, temperature of 20°C, and volume of 500 cm³?

A

1.46 g

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
65
Q

Calculate the molar mass (Mr) of a volatile liquid if 0.150 g is injected into a gas syringe at 70°C and 100 kPa with a volume of 80 cm³.

A

53.4 g mol-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
66
Q

What are potential errors when using a gas syringe?

A
  • Gas escapes before bung inserted
  • Syringe sticks
  • Some gases are soluble in water
67
Q

What is the molar gas volume at room temperature and pressure?

68
Q

How can the pressure of a gas mixture in a flask be calculated?

A

Use P1V1 = P2V2

69
Q

True or False: Equal volumes of any gases contain equal numbers of molecules under the same conditions of temperature and pressure.

70
Q

What is the total volume of gases produced when 500 cm³ of CO reacts with 500 cm³ of NO?

71
Q

Calculate the volume of oxygen needed to react with 500 cm³ of methane.

72
Q

Fill in the blank: The volume of a gas depends on _______ and _______.

A

[pressure], [temperature]

73
Q

What does an acid release in aqueous solution?

74
Q

What are the most common strong acids?

A
  • Hydrochloric (HCl)
  • Sulfuric (H2SO4)
  • Nitric (HNO3)
75
Q

What is a weak acid example?

A

Ethanoic acid (CH3COOH)

76
Q

How is a Bronsted-Lowry acid defined?

A

As a proton (H+) donor

77
Q

What is the definition of a base?

A

Substances that neutralise acids

78
Q

What are common bases?

A
  • Metal oxides
  • Metal hydroxides
  • Ammonia
79
Q

How is a Bronsted-Lowry base defined?

A

As a proton (H+) acceptor

80
Q

What is an alkali?

A

A soluble base that releases OH- ions in aqueous solution

81
Q

What are the most common alkalis?

A
  • Sodium hydroxide (NaOH)
  • Potassium hydroxide (KOH)
  • Aqueous ammonia (NH3)
82
Q

What happens when a base accepts H+ ions?

A

It forms water (H2O)

83
Q

What is the difference between strong and weak acids?

A
  • Strong acids completely dissociate in water
  • Weak acids only slightly dissociate
84
Q

What is formed in a neutralisation reaction?

85
Q

How is a salt formed?

A

When the H+ ion of an acid is replaced by a metal ion or an ammonium ion

86
Q

What is the general equation for a neutralisation reaction?

A

ACID + BASE → SALT + WATER

87
Q

What is produced in acid and carbonate reactions?

A

Salt, Water, and Carbon Dioxide

88
Q

What indicates effervescence in carbonate reactions?

A

CO2 gas evolved

89
Q

What are the safety precautions for conducting titrations?

A
  • Rinse equipment
  • Wear eye protection and gloves
  • Wash affected parts after spillage
90
Q

What is the purpose of using indicators in titrations?

A

To observe colour change at the end point

91
Q

What color change does phenolphthalein indicate?

A

Pink (alkali) to colourless (acid)

92
Q

What color change does methyl orange indicate?

A

Yellow (alkali) to red (acid)

93
Q

What should be done if the jet space in the burette is not filled properly?

A

It can lead to errors in titre readings

94
Q

What is required for titration results to be considered accurate and repeatable?

A

Two concordant results within 0.1 cm³ of each other

95
Q

What should be recorded during a titration?

A
  • Initial and final readings
  • Titre volumes to 2 decimal places
96
Q

What is the effect of adding distilled water during a titration?

A

It washes acid into the reaction mixture without affecting the titration reading

97
Q

What are common titration equations?

A
  • CH3COOH + NaOH → CH3COO-Na+ + H2O
  • H2SO4 + 2NaOH → Na2SO4 + 2H2O
  • HCl + NaOH → NaCl + H2O
98
Q

What should be considered when titrating a mixture?

A

Whether the mixture contains other substances with acid-base properties

99
Q

Why are sodium hydrogen carbonate and calcium carbonate used for neutralising excess acid?

A

They are not corrosive and have no toxicity

100
Q

What is a suitable substance for dealing with excess stomach acid?

A

Magnesium hydroxide

101
Q

True or False: Acids and alkalis are corrosive.

102
Q

What is the definition of ‘Readings’ in the context of measurements?

A

The values found from a single judgement when using a piece of equipment.

103
Q

How are ‘Measurements’ defined?

A

The values taken as the difference between the judgements of two values.

104
Q

What is the sensitivity uncertainty for a 3 d.p. balance?

A

+ 0.001 g.

105
Q

What is the sensitivity uncertainty for a volumetric flask?

A

+ 0.1 cm3.

106
Q

What is the sensitivity uncertainty for a 25 cm pipette?

A

+ 0.1 cm3.

107
Q

What is the sensitivity uncertainty for a burette?

A

+ 0.10 cm3.

108
Q

How do you calculate percentage error for a piece of equipment?

A

% uncertainty = (uncertainty / measurement made on apparatus) × 100.

109
Q

What is the formula to calculate % uncertainty for a burette?

A

% uncertainty = 0.10 / average titre result × 100.

110
Q

What is the method to find the maximum percentage apparatus uncertainty?

A

Add all the individual equipment uncertainties together.

111
Q

What is the uncertainty for an analogue scale reading?

A

At least ±0.5 of the smallest scale reading.

112
Q

What is the uncertainty for an analogue scale measurement?

A

At least ±1 of the smallest scale reading.

113
Q

What is the uncertainty for a digital scale?

A

± the resolution of the apparatus in each measurement.

114
Q

What is the uncertainty of a measurement using a burette during titration?

A

+/- 0.10 cm3 for two readings.

115
Q

How can uncertainties in a titration be reduced?

A

Replace measuring cylinders with pipettes or burettes.

116
Q

What effect does increasing the titre volume have on % uncertainty?

A

It reduces the % uncertainty in a burette reading.

117
Q

How can you decrease apparatus uncertainties?

A
  • Decrease the sensitivity uncertainty by using apparatus with greater resolution
  • Increase the size of the measurement made.
118
Q

In an investigation, which measurements have the highest experimental uncertainties?

A

The experiments with the smallest readings.

119
Q

How can you reduce % uncertainty in weighing a solid?

A

Use a balance that measures to more decimal places or use a larger mass.

120
Q

What is the method for calculating the percentage difference between actual and calculated values?

A

% = (difference / actual value) × 100.

121
Q

If the calculated Mr is 203 and the real value is 214, what is the % difference?

A

% = (11 / 214) × 100 = 5.41%.

122
Q

What does it indicate if the % uncertainty due to the apparatus is less than the percentage difference?

A

There is a discrepancy in the result due to other errors.

123
Q

What does it indicate if the % uncertainty due to the apparatus is greater than the percentage difference?

A

There is no discrepancy and all errors can be explained by the sensitivity of the equipment.

124
Q

What is the process of electron loss called?

A

Oxidation

Oxidation involves an increase in oxidation number.

125
Q

What happens to the oxidation number during oxidation?

A

It increases

Oxidation is characterized by electron loss.

126
Q

What is the oxidation number of all uncombined elements?

A

Zero

This is one of the rules for assigning oxidation numbers.

127
Q

What do the oxidation numbers of the elements in a compound add up to?

A

Zero

This follows the rules for determining oxidation numbers.

128
Q

What is the oxidation number of a monoatomic ion equal to?

A

The ionic charge

This is a rule for assigning oxidation numbers.

129
Q

In a polyatomic ion, what does the sum of the individual oxidation numbers equal?

A

The charge on the ion

This helps determine oxidation numbers in complex ions.

130
Q

What is the oxidation number of Group 1 metals?

A

+1

This is a specific rule for oxidation numbers.

131
Q

What is the oxidation number of Group 2 metals?

A

+2

This is part of the rules for assigning oxidation numbers.

132
Q

What is the oxidation number of Aluminum (Al)?

A

+3

This is a specific rule for oxidation numbers.

133
Q

What is the oxidation number of hydrogen (H) in most compounds?

A

+1

Except in metal hydrides where it is -1.

134
Q

What is the oxidation number of fluorine (F)?

A

-1

This is a fixed oxidation number for fluorine.

135
Q

What is the process of electron gain called?

A

Reduction

Reduction involves a decrease in oxidation number.

136
Q

What happens to the oxidation number during reduction?

A

It decreases

Reduction is characterized by electron gain.

137
Q

What is the oxidation number of sodium (Na) in NaCl?

A

+1

The chloride ion (Cl) has an oxidation number of -1.

138
Q

What is the oxidation number of chlorine (Cl) in NaCl?

A

-1

The oxidation numbers in NaCl sum to zero.

139
Q

What is the oxidation number of carbon (C) in CO3^2-?

A

+4

The carbonate ion has overall charge of -2.

140
Q

What is the oxidation number of oxygen (O) in CO3^2-?

A

-2

There are three oxygen atoms contributing to the charge.

141
Q

How do you find the oxidation number of an element with variable oxidation states?

A

Use oxidation number rules

This includes the rules for summing to zero or the charge.

142
Q

What is the oxidation number of chlorine (Cl) in CaCl2?

A

-1

There are two Cl atoms, each with an oxidation number of -1.

143
Q

What Roman numeral indicates the oxidation state of an element?

A

Magnitude of oxidation state

Used to clarify ambiguous names in compounds.

144
Q

What is the name of FeCl2?

A

Iron(II) Chloride

The Roman numeral indicates the +2 oxidation state of iron.

145
Q

What is the name of FeCl3?

A

Iron(III) Chloride

The Roman numeral indicates the +3 oxidation state of iron.

146
Q

What is the oxidation state of sulfur in K2SO4?

A

+6

The oxidation state is indicated in the compound’s name.

147
Q

Fill in the blank: NaClO is named __________.

A

Sodium chlorate(I)

The Roman numeral indicates the oxidation state of chlorine.

148
Q

Fill in the blank: K2SO4 is named __________.

A

Potassium sulfate(VI)

The Roman numeral indicates the oxidation state of sulfur.

149
Q

Fill in the blank: NaNO2 is named __________.

A

Sodium nitrate(III)

The Roman numeral indicates the oxidation state of nitrogen.

150
Q

Fill in the blank: NaNO3 is named __________.

A

Sodium nitrate(V)

The Roman numeral indicates the oxidation state of nitrogen.

151
Q

What do metals generally do in redox reactions?

A

Metals generally form ions by losing electrons with an increase in oxidation number to form positive ions.

Example: Zn → Zn2+ + 2e-

152
Q

What happens to the oxidation number of oxygen in redox reactions?

A

Oxygen is reducing because its oxidation number is decreasing from 0 to -2.

Example: 4Li + O2 → 2Li2O

153
Q

How do non-metals typically react in redox reactions?

A

Non-metals generally react by gaining electrons with a decrease in oxidation number to form negative ions.

Example: Cl + 2e → 2Cl-

154
Q

What is the change in oxidation number for tungsten in the reaction WO3 + 3H2 → W + 3H2O?

A

Tungsten is reducing because its oxidation number is decreasing from +6 to 0.

Oxidation states: +6 to 0

155
Q

What is the oxidation change for lithium in redox reactions?

A

Lithium is oxidising because its oxidation number is increasing from 0 to +1.

Example: 2Li → 2Li+ + 2e-

156
Q

What is the change in oxidation number for nitrogen in redox reactions?

A

Nitrogen is reducing because its oxidation number is decreasing from +5 to +4.

Example: 2Sr(NO3)2 → 2SrO + 4NO2 + O2

157
Q

What happens to hydrogen’s oxidation number in redox reactions?

A

Hydrogen is oxidising because its oxidation number is increasing from 0 to +1.

Example: 2NH3 + NaClO → N2H4 + NaCl + H2O

158
Q

What is the change in oxidation number for chlorine in redox reactions?

A

Chlorine is reducing because its oxidation number is decreasing from +1 to -1.

Example: 2NH3 + NaClO → N2H4 + NaCl + H2O

159
Q

How does oxygen behave in redox reactions?

A

Oxygen is oxidising because its oxidation number is increasing from -2 to 0.

Not all oxygen atoms change oxidation number in every reaction.

160
Q

What is the general reaction format for metals reacting with acids?

A

ACID + METAL → SALT + HYDROGEN.

Example: 2HCl + Mg → MgCl2 + H2

161
Q

What is the oxidation change for hydrogen in the reaction 2HCl + Mg → MgCl2 + H2?

A

Hydrogen is reducing because its oxidation number is decreasing from +1 to 0.

Oxidation states: +1 to 0

162
Q

What is the oxidation change for magnesium in reactions with acids?

A

Magnesium is oxidising because its oxidation number is increasing from 0 to +2.

Example: Mg → Mg2+ + 2e-

163
Q

What is the oxidation change for nitrogen in redox reactions?

A

Nitrogen is oxidising because its oxidation number is increasing from -3 to -2.

Example: In reactions with strong oxidisers.

164
Q

What observable effect occurs when metals react with hydrochloric acid?

A

These reactions will effervesce because H2 gas is evolved and the metal will dissolve.

Example: Fe + H2SO4 → FeSO4 + H2

Chemistry (6 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions