Concept explainers
Interpretation:
The value of
Concept introduction:
A buffer is defined as a solution which does not show any change in its
Acidic Buffer is a solution which has the
Basic Buffer is a solution which has the
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Chemistry & Chemical Reactivity
- 13. A 60.00 mL sample of 0.075 M sodium benzoate (NaC7H5O2) was titrated with 0.050 M HCl. What is the pH of the solutionafter 10.00 ml of HCl is added?(a) 4.19(b) 5.09(c) 5.74(d) 6.2414. What is the ratio of moles of benzoate (C7H5O2‒) to benzoic acid (HC7H5O2) in the solution that results from thecombination of the NaC7H5O2 and HCl in the problem above?(a) 8(b) 0.125(c) 0.0040(d) 0.00050arrow_forward100.0 mL 0.15 M aqueous HF (K₁ = 6.8 x 10-4) is mixed with 125.0 mL 0.23 M NaF. What is the pH of the resulting solution? (A) 2.17 (B) 3.17 (C) 3.35 (D) 3.45 a b Carrow_forwardCalculate the pH change that results when 15 mL of 2.0 M HCI is added to 580. mL of each of the following solutions (a) pure water 4.0-5.70 (b) 0.10 M CH3COO 4.04.28 (c) 0.10 M CH3COOH 4.0 (d) a solution that is 0.10 M in each CH3COO and CH3COOH. 4.0arrow_forward
- Calculate the pH change that results when 11 mL of 5.1 M NaOH is added to 790. mL of each the following solutions. Use the Acid-Base Table. (a) pure water 4.0 5.84 (b) 0.10 M NH4CI 4.0 5.43 (c) 0.10 M NH3 4.0✔ X (d) a solution that is 0.10 M in each NH4+ and NH3 4.0✔arrow_forwardCalculate the number of grams of ammonium chloride that must be added to 2.00 L of a 0.500 M ammonia solution to obtain a buffer of pH = 9.20. Assume the volume of the solution does not change as the solid is added. Kb for ammonia is 1.80 * 10-5. (a) 60.7 g (b) 30.4 g (c) 1.52 g (d) 0.568 g (e) 1.59 * 10-5arrow_forwardCalculate the pH change that results when 15 mL of 2.7 M HCI is added to 600. mL of each of the following solutions. Use the Acid-Base Table. (a) pure water 4.0 -5.82 (b) 0.10 M CH3COO- 4.0 4.43 (c) 0.10 M CH3COOH 4.0 X (d) a solution that is 0.10 M in each CH3COO and CH3COOH. 4.0arrow_forward
- How many moles of HCOONA must be added to 1.0 L of 0.10 M HCOOH to prepare a buffer solution with a pH of 3.4? (HCOOH K = 2 × 10 ) (A) 0.01 (B) 0.05 (C) 0.1 (D) 0.2 What is the percent ionization of a 0.10 M solution of formic acid at 25°C? Formic acid, HCOOH, has a Ka value of 1.9 x 104 at 25°C. (A) 0.19% (B) 1.4% (C) 4.4% (D) 14%arrow_forwardWhat is the pH of the following mixtures?(a) 0.025 M NaF(b) 0.35 M CH3NH3Cl (c) 0.2 KClO (d) 0.50 M NaCIO2arrow_forwardA buffer is made with sodium acetate (CH3COONa)and acetic acid (CH3COOH); the Ka for acetic acid is 1.80 * 10-5. The pH of the buffer is 3.98. What is the ratio of the equilibrium concentration of sodium acetate to that of acetic acid?(a) -0.760 (b) 0.174 (c) 0.840 (d) 5.75 (e) Not enough informa-tion is given to answer this question.arrow_forward
- Calculate the pH during the titration of 40.00 mL of 0.1000 M propanoic acid (HPr; Ka = 1.3x10-5) after each of the following additions of 0.1000 M NaOH:(a) 0.00 mL (b) 30.00 mL (c) 40.00 mL (d) 50.00 mLarrow_forwardCalculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after the following additions of base: (a) 28.00 mL (b) 39.50 mL (c) 52.00 mLarrow_forwardA 20.0 mL sample of 0.150 M ethylamine CH3CH2NH2 is titrated with 0.0981 M HCl. What is the pH after the addition of 0 mL HCl? pKb (CH3CH2NH2) = 3.25. (A) 10.75 (B) 11.04 (C) 2.96 (D) 11.46arrow_forward
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