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51 Cards in this Set
- Front
- Back
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Which of the following is characteristic of an acid? |
Has a sour taste |
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Identify the major ions present in an aqueous LiOH solution. |
Li+, OH- |
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Which of the following substances is NEVER a Brønsted-Lowry acid in an aqueous solution? |
Sodium acetate, NaCH3CO2(s) |
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Ammonium hydroxide is a weak base because it |
dissociates only slightly in water |
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Arrange the acids H2Se, H2Te, and H2S in order of increasing acid strength. |
H2S < H2Se < H2Te |
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Identify the conjugate base of HClO3 in the reaction ClO3- + HSO4- ↔ HClO3 + SO42- |
ClO3- |
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Predict the direction in which the equilibrium will lie for the reaction C6H5COO- + HF C6H5COOH + F-. Ka(C6H5COOH) = 6.5 x 10-5; Ka(HF) = 7.1 x 10-4 |
To the right |
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For H3PO4, Ka1 = 7.3 x 10-3, Ka2 = 6.2 x 10-6, and Ka3 = 4.8 x 10-13. An aqueous solution of NaH2PO4 therefore would be |
basic |
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Which of these salts will form a neutral solution on dissolving in water? |
NaCl |
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Arrange the following compounds in increasing order of pH. Assume all are 1.0 M solutions. (Ka HNO2 = 3.7 x 10-4; Kb NH3 = 1.8 x 10-5) NaCl NaOH HNO3 NH4Cl NaNO2 |
HNO3, NaNO2, NaCl, NH4Cl, NaOH |
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Identify the major ions present in an aqueous HNO3 solution. |
H+, NO3- |
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Which of following is true about strong acids? |
Strong acids are 100% ionized in water. |
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The pH of human blood is 7.30. What is the molar OH- concentration? |
2.0 x 10-7 M |
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What is the pH of 0.75 M HCl(aq) at 25oC? |
0.12 |
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What is the pH of a 0.014 M Ca(OH)2 solution? |
12.45 |
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A 0.10 M NH3 solution is 1.3% ionized. Calculate the H+ ion concentration. NH3 + H2O NH4+ + OH- |
7.7 x 10-12 M |
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What is the pH of 0.30 M aqueous formic acid? (Ka of HCO2H = 1.8 x 10–4) |
2.14 |
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A tablet of a common over-the-counter drug contains 2.00 x 102 mg of caffeine (C8H10N4O2; molar mass = 194.0 g/mol). What is the pH of the solution resulting from the dissolution of two of these tablets in 225. mL of water at 25oC? (For caffeine, Kb = 4.1 x 10-4.) |
11.24 |
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What is the chemical formula of the salt produced by the neutralization of potassium hydroxide with sulfuric acid? |
K2SO4 |
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Predict the direction in which the equilibrium will lie for the reaction |
To the left |
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What mass of sodium fluoride (FW=42.0 g/mol) must be added to 3.50 x 102 mL of water to give a solution with pH = 8.40? [Ka(HF) = 7.1 x 10-4] |
1.7 x 10-4 g |
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What is the pH of 0.50 M NaOCl if the Ka for HOCl is 3.5 x 10-8? |
10.6 |
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Which of the following corresponds to Ka2 for H2CO3? |
HCO3- ↔ CO3-2 + H+ |
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The OH- concentration in a bottle of an ammonia-based cleaner is 4.0 x 10-5 M. What is the pH of this cleaner? |
9.6 |
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Which solution will have the lowest pH? Ka (HCN) = 4.9 x 10-10Kb (NH3) = 1.8 x 10-5 |
0.10 M HNO3 |
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According to the Arrhenius concept, which of the following substances is NOT a base in aqueous solutions? |
NH3 |
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Which of the following is correctly identified? |
NaOH, strong base |
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When comparing acid strength of binary acids HX, as X varies within a particular group of the periodic table, which one of these factors dominates in affecting the acid strength? |
Bond strength |
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Seawater has a hydroxide ion concentration of 2.0 x 10-6 M. What is the pH of seawater? |
8.30 |
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The pH of an aqueous solution is 11.45. What is the OH- concentration? |
2.8 x 10-3 M |
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What is the pH of 0.250 M HCl? |
0.600 |
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What is the pH of 0.50 M aqueous ethylamine? (Kb of C2H5NH2 = 4.3 x 10–4) |
12.16 |
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What is the chemical formula of the salt produced by the neutralization of nitric acid with calcium hydroxide? |
Ca(NO3)2 |
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Which of the following chemical equations corresponds to Ka3 of phosphoric acid? |
HPO42–(aq) + H2O() PO43–(aq) + H3O+(aq) |
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Which of these salts will form an acidic solution upon dissolving in water? |
NH4Br |
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What is the pH of a 0.50 M solution of NaNO2? The Ka for HNO2 is 4.5 x 10-4. |
8.5 |
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What mass of sodium cyanide (FW=49.0 g/mol) must be added to 2.50 x 102 mL of water at 25oC in order to obtain a solution having a pH of 10.50? (Ka(HCN) = 4.9 x 10-10) |
0.066 g |
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All of the following acids are weak EXCEPT |
HNO3 |
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The conjugate base of H2O is |
OH- |
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The pH of vinegar is 3.0. What is the concentration of OH- in vinegar? |
1 x 10-3 M |
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Calculate the pH of a 6.71 x 10-2 M NaOH solution. |
12.83 |
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A tablet of a common over-the-counter drug contains 2.00 x 102 mg of caffeine (C8H10N4O2; molar mass = 194.0 g/mol). What is the pH of the solution resulting from the dissolution of two of these tablets in 225. mL of water at 25oC? (For caffeine, Kb = 4.1 x 10-4.) |
11.24 |
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Morphine, C17H19NO3 (MW=285.0 g/mol), is often used to control severe post-operative pain. What is the pH of the solution made by dissolving 25.0 mg of morphine in 1.00 x 102 mL of water at 25oC? (For morphine, Kb = 1.62 x 10-6.) |
9.57 |
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Which of the following chemical equations corresponds to Kb1 for SO32–? |
HSO3–(aq) + H2O() H2SO3(aq) + OH–(aq) |
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What mass of sodium nitrite (FW=69.0 g/mol) must be added to 3.50 x 102 mL of water to give a solution with pH = 8.40? [Ka(HNO2) = 5.6 x 10-4] |
8.5 g |
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Find the pH of a 0.200 M aqueous solution of acetic acid, for which Ka = 1.8 x 10-5. |
2.72 |
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The hydroxide ion concentration in a sample of lemon juice is 1.9 x 10-12 M. What is the pH? |
2.28 |
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A solution of formic acid is 0.47% ionized. What is the pH of a 0.33 M formic acid solution? |
2.52 |
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Which is NOT a characteristic property of acids? |
Reacts with metals to yield CO2 gas |
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Which of the following chemical equations corresponds to Ka2 of phosphoric acid? |
H2PO4–(aq) + H2O() HPO42–(aq) + H3O+(aq) |
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What mass of potassium hypochlorite (FW=90.6 g/mol) must be added to 4.50 x 102 mL of water to give a solution with pH = 10.20? [Ka(HClO) = 4.0 x 10-8] |
4.1 g |
