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
- Calculate the number of grams of ammonium chloride thatmust 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 thesolution does not change as the solid is added. Kb for ammoniais 1.80 x 10-5.(a) 60.7 g (b) 30.4 g (c) 1.52 g (d) 0.568 g(e) 1.59 x 10-5 garrow_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 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_forward
- Calculate 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_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 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_forwardCalculate 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_forward9. 15.00 mL of 0.100 M NaOH are added to 50.00 mL of a buffer solution containing 1.0 mmol CH3CO0H and 1.0 mmol CH3CO0. What is the new solution pH? (а) 11.89 (b) 2.11 (c) 7.87 (d) Can't tell / need more info.arrow_forward
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