Acid Bases And Salt Flashcards
1
Q
What is an Arrhenius acid?
A
A substance that dissociates in water to form hydrogen ions or protons.
2
Q
Give an example of an Arrhenius acid.
A
HCl → H + (aq) + Cl - (aq)
3
Q
What is an Arrhenius base?
A
A substance that dissociates in water to form hydroxide ions.
4
Q
Give an example of an Arrhenius base
A
Ca(OH)2 (s) → Ca++ (aq) + 2 OH- (aq)
5
Q
What is the Brønsted-Lowry theory?
A
Brønsted-Lowry acid: ‘A substance that can donate hydrogen ion (H+) is acid’ Brønsted-Lowry base: ‘A substance that can accept hydrogen ion (H+) is base’ Conjugate acid: an acid that forms when a base gains a proton. Conjugate base: a base that forms when an acid loses a proton.
6
Q
What is the Brønsted Lowry acid in the equation HNO3 (aq) + H2O (l) → H3O+ (aq) + NO3− (aq)?
A
HNO3
7
Q
What is the Brønsted Lowry acid in the equation CH3COOH (aq) + H2O (l) ⇌ H3O+ (aq) + CH3COO− (aq)?
A
CH3COOH
8
Q
What are the limitations of Arrhenius theory?
A
- It requires the solutions to be aqueous. 2. It only applies to substances that produce Hydrogen ions (H + ) or hydroxide ions (OH − ).
9
Q
What are the limitations of Brønsted-Lowry Concept?
A
- The protonic definition cannot be used to explain the reactions occuring in non - protonic solvents such as COCl 2 , SO 2 , N 2 O 4 , etc. 2. It cannot explain the reactions between acidic oxides and the basic oxides which take place even in the absence of the solvent e.g., There is no proton transfer in the above example. 3. It is failed to explain substances like BF 3 , AlCl 3 etc, do not have any hydrogen and hence cannot give a proton but are known to behave as acids.
10
Q
What are the Lewis concepts of acids and bases?
A
Lewis acid: ‘An acid is a substance (molecule or ion) that can accept a pair of electrons’. Lewis base: ‘An base is a substance (molecule or ion) that can donate a pair of electrons’.
11
Q
How is BF 3 classified as a Lewis acid?
A
B is member of group IIIA. It contains 3 valance electrons. It is sharing 3 electrons with F so 6 electron are with boron in valance shell, it can accept pair of electron to complete octet.
12
Q
What is the amphoteric nature of water?
A
The bonds between water molecules rapidly break and re-form, sometimes in an uneven way to give solvated H3O+ and solvated HO-.
13
Q
What is the abbreviation for the cation part in a solution?
A
H + (aq)
14
Q
What is the abbreviation for the anion part in a solution?
A
HO - (aq)
15
Q
What is the pH of neutral water?
A
7
16
Q
What are the physical properties of acids and bases?
A
Acids: Taste sour, frequently burn nose (conc), sticky, turn litmus paper blue to red, good conductors in ionic form, pH range 1 to 7, highly corrosive. Bases: Taste bitter, no smell except NH3, slippery, turn litmus paper red to blue, good conductors in ionic form, pH range 7 to 14, corrosive.
17
Q
What are the chemical properties of acids?
A
Acids react with bases or metallic hydroxide to form salt and water. This reaction is called neutralization reaction. General reaction: Acid + Base → Salt + Water. General reaction: Acid + Metal hydroxide → Salt + Water. An example is the neutralization reaction of nitric acid and sodium hydroxide: HNO3 (aq) + NaOH (s) → NaCl (aq) + H2O (g).
18
Q
What is the general reaction when acids react with metals?
A
Acid + Metal → Salt + Hydrogen gas
19
Q
What happens when acids react with metal oxides?
A
Acid + Metal oxide → Salt + water
20
Q
What is the general reaction when acids react with carbonates or bicarbonates?
A
Acid + Carbonate/Bicarbonate → Metallic Salt + water + carbon dioxide gas
21
Q
What is the chemical equation for the reaction of carbon dioxide with sodium hydroxide?
A
CO2 + 2NaOH → Na2CO3 + H2O
22
Q
What is the general reaction when a base reacts with a non-metallic oxide?
A
Base + non-metallic oxides → Salt + water
23
Q
What is the chemical equation for the reaction of ammonium chloride with sodium hydroxide?
A
NH4Cl + NaOH → NH3 + NaCl + H2O
24
Q
What is the general reaction when a base reacts with an ammonium salt?
A
Base + Ammonium salt → Salt + Ammonia gas + Water
25
What is the chemical equation for the reaction of zinc sulphate solution with sodium hydroxide?
ZnSO4(aq) + 2NaOH(aq) → Zn(OH)2(s) + Na2SO4(aq)
26
What is basicity of acid?
Ability of an acid to consume the no of hydroxide ions (OH - ) during a chemical reaction. Or The no of ionizable hydrogen (H + ) ions present in one molecule of an acid is called it’s basicity.
27
Define Monobasic Acid
1 molecule produce 1 H + ion upon dissociation and can consume one OH - Example: HCl, HNO3
28
Define Dibasic Acid
1 molecule produce 2 H+ ion upon dissociation and can consume two OH - . Example: H2SO4
29
What is acidity of base?
Ability of base to consume the number of Hydrogen ions (H + ) during a chemical reaction. Or The no of ionizable hydroxide ions (OH - ) present in one molecule of a base is called acidity.
30
Define Monoprotic base
1 molecule produce 1 OH - ion upon dissociation and can consume one H + Example: NaOH, KOH
31
What is a diprotic base?
1 molecule produce 2 OH- ion upon dissociation and can consume two H+.
32
Provide an example of a diprotic base.
Ca(OH)2, Mg(OH)2
33
What is the dissociation equation for Ca(OH)2?
Ca(OH)2(aq) -> Ca++(aq) + 2OH-(aq)
34
What are weak acids and bases?
Those acids and bases which cannot completely ionize in aqueous solution but show partial ionization.
35
Provide examples of common weak acids and bases.
Common Weak Acids: Formic (HCOOH), Acetic (CH3COOH), Trichloroacetic (CCl3COOH), Hydrofluoric (HF), Hydrocyanic (HCN), Hydrogen sulfide (H2S). Common Weak Bases: Ammonia (NH3), trimethyl ammonia (N(CH3)3), Pyridine (C5H5), ammonium hydroxide (NH4OH), Water (H2O), conjugate bases of weak acids (HCOO-), conjugate acids of weak bases (NH+4), Blood.
36
What are strong acids and bases?
Strong acids and bases are those acids and bases which show complete ionization in aqueous medium.
37
What are some common strong acids?
Hydrochloric Acid (HCl), Sulphuric acid (H2SO4), Hydrobromic Acid (HBr), Nitric acid (HNO3), HydroIodic acid (HI), Hypochloric acid (HClO3)
38
What are some common strong bases?
Sodium hydroxide (NaOH), Calcium hydroxide (Ca(OH)2), Magnesium hydroxide (Mg(OH)2), Lithium hydroxide (LiOH), Barium hydroxide (Ba(OH)2), Strontium hydroxide (Sr(OH)2)
39
What is etching?
Etching is the process of using strong acid to cut into the unprotected parts of a metal surface or glass to create a design on them. It is the most important technique for old master prints, and remains widely used today. In pure etching, a metal (usually copper, zinc or steel) plate or galss is covered with a waxy ground, which is resistant to acid. The artist then scratches off the ground with a pointed etching needle where he/she wants a line to appear in the finished piece, so exposing the bare metal/glass. The plate is then dipped in a bath of acid. The acid "bites" into the metal/glass, where it is exposed, leaving behind lines sunk into the plate. The remaining ground is then cleaned off the plate. The plate is inked all over, and then the ink wiped off the surface, leaving only the ink in the etched lines.
40
What is the most important technique for old master prints?
Etching
41
What happens after the plate is dipped in a bath of acid during the etching process?
The acid 'bites' into the metal/glass, where it is exposed, leaving behind lines sunk into the plate. The remaining ground is then cleaned off the plate.
42
What is the final step in the etching process?
The plate is inked all over, and then the ink wiped off the surface, leaving only the ink in the etched lines.
43
What is pH?
pH is the negative logarithm of molar concentration of H+ ions.
44
How is pH measured using pH paper and pH meter?
pH paper is used to determine the acidic or basic nature of a solution by the change in color, while a pH meter consists of a pH electrode connected to a meter and provides a more reliable and accurate measurement of pH.
45
Calculate the pH of 0.04M NaOH solution
pH= 12.6
46
Find the pH and the pOH of a 0.023 M solution of hydrochloric acid
pH: 1.63, pOH: 12.37
47
Find the pH and the pOH of a 6.6 x 10^-6 M solution of nitric acid
pH: 5.18, pOH: 8.82
48
Find the pH and the pOH of a 0.0334 M solution of potassium hydroxide
pH: 13.48, pOH: 0.52
49
Find the pH and the pOH of a 1.0 x 10^-5 M solution of hydro arsenic acid
pH: 4.00, pOH: 10.00
50
Find the pH and the pOH of a 2.23 x 10^-2 M solution of aluminum hydroxide
pH: 12.65, pOH: 1.35
51
What is the molarity of the magnesium hydroxide solution?
0.000901 M
52
What is the molarity of the hydrosulfuric acid solution?
7.23 x 10^-5 M
53
What is the molarity of the hydrochloric acid solution?
2.58 x 10^-6 M
54
What is the molarity of the sodium hydroxide solution?
0.000469 M
55
What is the molarity of the sulfuric acid solution?
0.000896 M
56
It takes 83 mL of a 0.45 M NaOH solution to neutralize 235 mL of an HCl solution. What is the concentration of the HCl solution?
The concentration of the HCl solution is 1.26 M
57
You are titrating an acid into a base to determine the concentration of the base. The endpoint of the neutralization is reached but the stopcock on the buret sticks slightly and allows a few more drops of acid to fall into the solution. How will this affect your calculations for the concentration of the base?
The additional drops of acid will increase the calculated concentration of the base
58
It takes 38 mL of 0.75 M NaOH solution to completely neutralize 155 mL of a sulfuric acid solution (H2SO4). What is the concentration of the H2SO4 solution?
The concentration of the H2SO4 solution is 1.84 M
59
Will the small amount of water left in the buret affect the determined value for the concentration of the acid when titrating a base into an acid solution?
Yes, it will affect the determined value. The water will dilute the acid solution, resulting in a lower concentration of the acid.
60
What is the concentration of the NaOH solution if it takes 12.5 mL of a 0.30 M HCl solution to neutralize 285 mL of NaOH solution?
The concentration of the NaOH solution is 0.105 M.
61
Is the solution formed from the contents of the two test tubes acidic or basic? What is the pH of the resulting solution?
The solution is acidic. The pH of the resulting solution can be calculated using the concentrations of the NaOH and HCl solutions.
62
Write the balanced chemical equations and type of reaction for the neutralization reactions between HI and NaOH
HI + NaOH -> NaI + H2O, double displacement reaction
63
Write the balanced chemical equations and type of reaction for the neutralization reactions between H2CO3 and Sr(OH)2
H2CO3 + Sr(OH)2 -> SrCO3 + 2H2O, double displacement reaction
64
Write the balanced chemical equations and type of reaction for the neutralization reactions between Ca(OH)2 and H3PO4
3Ca(OH)2 + 2H3PO4 -> Ca3(PO4)2 + 6H2O, double displacement reaction
65
Write the balanced chemical equations and type of reaction for the neutralization reactions between hydrobromic acid and barium hydroxide
2HBr + Ba(OH)2 -> 2H2O + BaBr2, double displacement reaction
66
Write the balanced chemical equations and type of reaction for the neutralization reactions between zinc hydroxide and nitric acid
Zn(OH)2 + 2HNO3 -> Zn(NO3)2 + 2H2O, double displacement reaction
67
Write the balanced chemical equations and type of reaction for the neutralization reactions between aluminum hydroxide and hydrochloric acid
Al(OH)3 + 3HCl -> AlCl3 + 3H2O, double displacement reaction
68
Complete and balance the following equations representing neutralization reactions: CsOH + H2CO3
2CsOH + H2CO3 -> Cs2CO3 + 2H2O, double displacement reaction
69
Complete and balance the following equations representing neutralization reactions: HF + Mg(OH)2
2HF + Mg(OH)2 -> MgF2 + 2H2O, double displacement reaction
70
Complete and balance the following equations representing neutralization reactions: HNO3 + Al(OH)3
Al(OH)3 + 3HNO3 -> Al(NO3)3 + 3H2O, double displacement reaction
71
Complete and balance the following equations representing neutralization reactions: HCl + KOH
HCl + KOH -> KCl + H2O, double displacement reaction
72
Complete and balance the following equations representing neutralization reactions: HBrO3 + LiOH
LiOH + HBrO3 -> LiBrO3 + H2O, double displacement reaction
73
Give the name and the formula of the ionic compound produced by neutralization reactions between the following acids and bases; complete the missing information in given table. Acid and Base reactants
a) nitric acid and sodium hydroxide - sodium nitrate - NaNO3 b) hydroiodic acid and calcium hydroxide - CaI2 c) magnesium hydroxide and hydrosulfuric acid - magnesium sulfide d) ammonium hydroxide and hydrofluoric acid - NH4F e) barium hydroxide and sulfuric acid - barium sulfate f) chloric acid and rubidium hydroxide - rubidium chlorate - RbClO3 g) calcium hydroxide and carbonic acid
74
For each of the following ionic compounds, identify the acid or base that reacted. Salt
a) NaCl - HCl b) Ca3(PO4)2 - Ca(OH)2 c) Zn(NO3)2 - HNO3 d) Al(ClO)3 - Al(OH)3 e) NH4I - HI
75
What is the definition of a salt?
Ionic compound formed by neutralization of acid and base is known as salt.
76
What are the properties of salts?
Salts are ionic in nature, have oppositely charged ions, are good conductors of electricity in dissolved or molten form, are brittle, hard and crystalline solids, can be white or have characteristic colors, are odorless and mostly have a salty taste, and have specific solubility properties in water.
77
How are soluble and insoluble salts prepared?
Preparation of soluble salts is carried out by the same methods as the chemical properties of acids and bases, including reactions of acid with base, carbonates, metal, and basic oxides.
78
How do you determine whether a salt is soluble or insoluble in water?
By knowing certain facts such as the solubility of sodium, potassium, and ammonium salts, nitrate salts, common chloride salts, common sulfate salts, and metal hydroxides in water.
79
What is the definition of a salt?
Ionic compound formed by neutralization of acid and base is known as salt
80
What are the properties of salts?
Salts are ionic in nature, have oppositely charged ions, are good conductors of electricity in dissolved or molten form, are brittle, hard and crystalline solids, can be white or have characteristic colors, are odorless and mostly have a salty taste, and have specific solubility properties in water.
81
How are soluble salts prepared?
Preparation of soluble salts is carried out by the same methods as the chemical properties of acids and bases, including reactions of acid with base, carbonates, metal, and basic oxides.
82
What are some examples of salts that are soluble in water?
Examples include Na2CO3, K2SO4, NH4Cl, Mg(NO3)2, Cu(NO3)2, Fe(NO3)3, and sodium, potassium, and ammonium carbonates.
82
How do you determine whether a salt is soluble or insoluble in water?
By knowing certain facts such as the solubility of sodium, potassium, and ammonium salts, nitrate salts, common chloride salts, common sulfate salts, and metal hydroxides in water.
83
What are some examples of salts that are insoluble in water?
Examples include AgCl, PbCl2, PbSO4, BaSO4, CaSO4, and metal hydroxides other than NaOH, KOH, and NH4OH.
84
What are normal salts?
Normal salts are electrically neutral and are formed when acids and bases neutralize. They don’t have replaceable hydrogen or hydroxyl in their formula.
85
What are basic salts?
Basic salts are formed due to partial replacement of hydroxy radicals of a diacidic base or a triacidic base with an acid radical. They consist of hydroxyl, metallic cation, and anion of an acid.
86
What are acidic salts?
Acidic salts are produced by the replacement of only a part of the acidic hydrogen of the polybasic acid by a metal. They can further be neutralized by reacting with a base.
87
What are double salts?
Double salts have more than one cation or anion. They are a crystalline salt having the composition of a mixture of two simple salts but with a different crystal structure from either.
88
What are mixed salts?
Mixed salts are made from more than one base or acid.
89
What are complex salts?
Salt formed due to combining a saturated solution of simple salts followed by crystallization of the solution similar to double salts. For e.g. Sodium silver cyanide Na2[Ag(CN)2], hexacyano iron III chloride [Fe(CN)6]Cl3
90
What are the uses of sodium chloride or common salt (NaCl)?
1. Used in cooking food as well as for cooking gas. 2. Used as a preservative in pickles and in curing meat and fish. 3. Used in the manufacture of soap. 4. Used to melt the ice in winter in cold countries. 5. Used for making chemical likes washing Soda, baking soda etc.
91
What are the uses of sodium carbonate or washing soda (Na2CO3.10H2O)?
1. Used as cleansing agent. 2. Used for removing permanent hardness of water. 3. Used in the manufacturing of glass, soap and paper.
92
What are the uses of baking soda or sodium bi-carbonate (NaHCO3)?
1. Used as neutralising agent (antacid). 2. Used for making baking powder. 3. Used in fire extinguisher.
93
What are the uses of bleaching powder or calcium hypochlorite?
1. Used as bleaching agent in cotton industry and paper industry for bleaching cotton and linen as well as wood pulp respectively. 2. Used for disinfecting drinking water. 3. Used for making chloroform (CHCl3). 4. Used for making the wool unshrinkable.
94
What are the uses of plaster of Paris or hemihydrate calcium sulphate, CaSO4 1/2 H2O?
1. Used in hospital for setting fractured bone. 2. Used for making toys, decoration material cheap ornament, chalk etc. 3. Used for fire-proofing material. 4. Used for making surface smooth.
