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10. Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is suitable for m...
8. What is the pH of a 5.00 x 102 M Ba(OH)2(aq) solution at room temperature?...
8. What is the pH of a 5.00 x 102 M Ba(OH)2(aq) solution at room temperature? a. 1.00 b. 1.30 c. 12.02 d. 12.70 e. 13.00 9. Assuming equal concentrations of conjugate acid and base, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 4.6-4.8? a. CH3COONa/CH3COOH (K = 1.8 x 105) b. NH/NHACI (K = 5.6 x 10-1) c. NaOCI/HOCI (Ka = 3.2 x 108) d. NaNO2/HNO2 (Ka = 4.5...
1. 200 mL of an aqueous solution contains 0.030 M concentrations of both Pb2+ and Ag+....
1. 200 mL of an aqueous solution contains 0.030 M
concentrations of both Pb2+ and Ag+. If 100
mL of 6.0 x 10-2 M NaCl is added to this solution will a
precipitate form? If so, what will the
precipitate be? The Ksp values for PbCl2 and AgCl are 1.7 x
10-5 and 1.8 x 10-10] 2. Which of the following is the expression
for the solubility product of Ba3(AsO4)2? 3. The pKa of a weak acid
is 6.50. What...
3,10 3. The pH of coffee is approximately 5.0. How many times greater is the [HO]...
3,10
3. The pH of coffee is approximately 5.0. How many times greater is the [HO] in coffee than in tap water having a pH of 8.0? Determine the plH of a KOH solution made by mixing 0.251 g KOH with enough water to make 1.0x102 mL of solution. 8. A) 0.62 B) 1.6 C) 30 D) 1,000 A) 1.35 B) 2.35 C) 7.00 D) 12.65 9. Assuming equal concentrations of conjugate base and acid, which one of the following...
10. Which of the following mixtures has lower pH a) Equal volumes of 0.10M HCIO, and...
10. Which of the following mixtures has lower pH a) Equal volumes of 0.10M HCIO, and 0.10M NaOH b) Equal volumes of 0.10M HCIO and 0.10M NH Ans: 1. Does the pH increase, decrease or remain same on addition of each of the following a) NH4NO) to NHs solution Ans: b) Na:CO) to NaHCO3 solution Ans: c) NaCIO4 to NaOH solution Ans: 12. Which of the following solutions give a buffer solution when equal volumes are mixed? a) 0.10M NaF...
All of the following are acid-base conjugate pairs EXCEPT Group of answer choices H2O, H3O+ NH4+,...
All of the following are acid-base conjugate pairs EXCEPT Group of answer choices H2O, H3O+ NH4+, NH3 CH3COOH, CH3COO- H3O+, OH- HPO42-, PO43- The pH of a 1.86 M solution of a weak monoprotic acid, is 2.31. What is the Ka of the acid? Group of answer choices 4.7 x 10-5 4.1 x 10-7 3.4 x 105 2.4 x 10-4 1.3 x 10-5 You have 250.0 mL of a 0.56 M solution of NaCH3COO. How many milliliters of a 0.50...
DNH ANH IB HU 12 Which species is the conjugate acid of NH3? A NH₂ BH,0...
DNH ANH IB HU 12 Which species is the conjugate acid of NH3? A NH₂ BH,0 | CNH 13 Which species is a diprotic acid? A Mg(OH)2 CH₂ BCH COOH DH,CO 14 Which compound is an example of weak acid? HNO3 в | HBr IC CHCOOH DH,SO, 15 Ammonia, NH, is an example of a.......? Strong acid B Strong base Icl Weak acid Weak base 16 Which ion is the strongest base? LA Br BF cr DNO, 17 Rank the...
1. Identify the Brönsted acid and base in the following reaction, and identify the conjugate base...
1. Identify the Brönsted acid and base in the following reaction, and identify the conjugate base and acid formed. HSO3-(aq) + CH3NH3(aq) ------ H2SO3(aq) + CH3NH2(aq) 2. Write the formulae for the conjugate acids of: 1. a) C2042: the oxalate ion. 2.b) C6H5NH2, aniline. 3.c)NH2OH, hydroxylamine. (Use above question as a guide for where to put the H.) 3. Calculate the molarity of OH' in solutions with the following concentrations of H30*: a) 0.020 mol LP b) 1.0 x 10-5...
Question 7 0.77 pts Title q7a7 Which of the following pairs of species, when mixed together in water in proper ratios,...
Question 7 0.77 pts Title q7a7 Which of the following pairs of species, when mixed together in water in proper ratios, would provide a buffer solution? Think each pair through very carefully in terms what species will form when they dissolve in water, and how they can then (potentially) react with water Refer to the table of strong acids/bases on the exam information sheet if you don't have them memorized yet. () KOH and NH4CI (ii)HCI and NH4CI (liI) NH3...
Acid Substance or Species HE HNO2 CH3COOH HOCI HOBI ka = 7.2 x 10-4 NH3 K...
Acid Substance or Species HE HNO2 CH3COOH HOCI HOBI ka = 7.2 x 10-4 NH3 K = 4.5 x 10-4 (CH3)3N = 1.8 x 10-5 [Co(OH)]2+ Ka = 3.5 x 10-8 [Fe(OH2)2]2+ Ka = 2.5 x 10-9 [Fe(OH2)613+ Ka = 3.5 x 10-4 [Be(OH)412+ Ka = 4.0 x 10–10 [Cu(OH)212+ Ka1 = very large HBO2 Ka2 = 1.2 x 10-2 (COOH)2 HOCN HCN H2SO4 Kb = 1.8 x 10-5 Kb = 7.4 x 10-5 Ka = 5.0 x 10-10 Ka...
QUESTION 11 Which of the following acid/base conjugate pairs could you use to make a buffer...
QUESTION 11 Which of the following acid/base conjugate pairs could you use to make a buffer solution with a pH of 2.10? The Kfor the acids are given in parentheses. Chlorous acid / chlorite (Ka = 1.1 10-2) Benzoic acid / benzoate (K, -6.3 * 10-5) O Hydrofluoric acid / fluoride (Ka = 6.6 x 10-4) Hydrogen phosphate / phosphate (Kg = 4.2 x 10-13) Ammonium / ammonia (K, -5.8 * 10-10)
8. What is the pH of a 5.00 x 102 M Ba(OH)2(aq) solution at room temperature? a. 1.00 b. 1.30 c. 12.02 d. 12.70 e. 13.00 9. Assuming equal concentrations of conjugate acid and base, which one of the following mixtures is suitable for making a buffer solution with an optimum pH of 4.6-4.8? a. CH3COONa/CH3COOH (K = 1.8 x 105) b. NH/NHACI (K = 5.6 x 10-1) c. NaOCI/HOCI (Ka = 3.2 x 108) d. NaNO2/HNO2 (Ka = 4.5...
1. 200 mL of an aqueous solution contains 0.030 M
concentrations of both Pb2+ and Ag+. If 100
mL of 6.0 x 10-2 M NaCl is added to this solution will a
precipitate form? If so, what will the
precipitate be? The Ksp values for PbCl2 and AgCl are 1.7 x
10-5 and 1.8 x 10-10] 2. Which of the following is the expression
for the solubility product of Ba3(AsO4)2? 3. The pKa of a weak acid
is 6.50. What...
3,10
3. The pH of coffee is approximately 5.0. How many times greater is the [HO] in coffee than in tap water having a pH of 8.0? Determine the plH of a KOH solution made by mixing 0.251 g KOH with enough water to make 1.0x102 mL of solution. 8. A) 0.62 B) 1.6 C) 30 D) 1,000 A) 1.35 B) 2.35 C) 7.00 D) 12.65 9. Assuming equal concentrations of conjugate base and acid, which one of the following...
10. Which of the following mixtures has lower pH a) Equal volumes of 0.10M HCIO, and 0.10M NaOH b) Equal volumes of 0.10M HCIO and 0.10M NH Ans: 1. Does the pH increase, decrease or remain same on addition of each of the following a) NH4NO) to NHs solution Ans: b) Na:CO) to NaHCO3 solution Ans: c) NaCIO4 to NaOH solution Ans: 12. Which of the following solutions give a buffer solution when equal volumes are mixed? a) 0.10M NaF...
DNH ANH IB HU 12 Which species is the conjugate acid of NH3? A NH₂ BH,0 | CNH 13 Which species is a diprotic acid? A Mg(OH)2 CH₂ BCH COOH DH,CO 14 Which compound is an example of weak acid? HNO3 в | HBr IC CHCOOH DH,SO, 15 Ammonia, NH, is an example of a.......? Strong acid B Strong base Icl Weak acid Weak base 16 Which ion is the strongest base? LA Br BF cr DNO, 17 Rank the...
1. Identify the Brönsted acid and base in the following reaction, and identify the conjugate base and acid formed. HSO3-(aq) + CH3NH3(aq) ------ H2SO3(aq) + CH3NH2(aq) 2. Write the formulae for the conjugate acids of: 1. a) C2042: the oxalate ion. 2.b) C6H5NH2, aniline. 3.c)NH2OH, hydroxylamine. (Use above question as a guide for where to put the H.) 3. Calculate the molarity of OH' in solutions with the following concentrations of H30*: a) 0.020 mol LP b) 1.0 x 10-5...
Question 7 0.77 pts Title q7a7 Which of the following pairs of species, when mixed together in water in proper ratios, would provide a buffer solution? Think each pair through very carefully in terms what species will form when they dissolve in water, and how they can then (potentially) react with water Refer to the table of strong acids/bases on the exam information sheet if you don't have them memorized yet. () KOH and NH4CI (ii)HCI and NH4CI (liI) NH3...
Acid Substance or Species HE HNO2 CH3COOH HOCI HOBI ka = 7.2 x 10-4 NH3 K = 4.5 x 10-4 (CH3)3N = 1.8 x 10-5 [Co(OH)]2+ Ka = 3.5 x 10-8 [Fe(OH2)2]2+ Ka = 2.5 x 10-9 [Fe(OH2)613+ Ka = 3.5 x 10-4 [Be(OH)412+ Ka = 4.0 x 10–10 [Cu(OH)212+ Ka1 = very large HBO2 Ka2 = 1.2 x 10-2 (COOH)2 HOCN HCN H2SO4 Kb = 1.8 x 10-5 Kb = 7.4 x 10-5 Ka = 5.0 x 10-10 Ka...
QUESTION 11 Which of the following acid/base conjugate pairs could you use to make a buffer solution with a pH of 2.10? The Kfor the acids are given in parentheses. Chlorous acid / chlorite (Ka = 1.1 10-2) Benzoic acid / benzoate (K, -6.3 * 10-5) O Hydrofluoric acid / fluoride (Ka = 6.6 x 10-4) Hydrogen phosphate / phosphate (Kg = 4.2 x 10-13) Ammonium / ammonia (K, -5.8 * 10-10)
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