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How much 6.01 M NaOH must be added to 620.0 mL of a buffer that is 0.0195 M acetic acid and 0.0230 M sodium acetate to raise the pH to 5.75?
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- A chemistry graduate student is given 500. mL of a 1.80M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K,= 4.9 x 10 – 10 What mass of KCN should the student dissolve in the HCN solution to turn it into a buffer with pH =9.70? You may assume that the volume of the solution doesn't change when the KCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 国 国 回A chemistry graduate student is given 450. mL of a 1.70M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K,= 4.9 × 10 ". What mass of KCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 8.97? You may assume that the volume of the solution doesn't change when the KCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.A chemistry graduate student is given 100. mL of a 0.90M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K,=4.9 × 10 10 What mass of KCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 8.97? You may assume that the volume of the solution doesn't change when the KCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
- A chemistry graduate student is given 300. mL of a 1.70 M pyridine (C,H,N) solution. Pyridine is a weak base with K,= 1.7 × 10. What mass of C,H,NHB1 should the student dissolve in the C,H,N solution to turn it into a buffer with pH = 4.87? You may assume that the volume of the solution doesn't change when the C,H,NHB1 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.6A chemistry graduate student is given 250. mL of a 1.40M ammonia (NH3) solution. Ammonia is a weak base with K-1.8x10 should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.17? What mass of NH, Br You may assume that the volume of the solution doesn't change when the NH4Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ?
- In a titration of 41.34 mL of 0.3483 M ammonia with 0.3483 M aqueous nitric acid, what is the pH of the solution when 41.34 mL of the acid have been added?A chemistry graduate student is given 500. mL of a 0.40 M ammonia (NH3) solution. Ammonia is a weak base with Kb=1.8x 10^-5 . What mass of NH4C1 should the student dissolve in the NH3 solution to turn it into a buffer with pH = 8.85? You may assume that the volume of the solution doesn't change when the NH, C1 is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.A buffer is formed by adding 1.0 mol of trimethylamine, (CH3)3N, and 1.0 mol of trimethylammonium, (CH3)3NH", in a 1.0 L container. If a 10.0 mL sample of this buffer is diluted to 1000 mL with water, what is the pH of the diluted buffer? For trimethylamine, K, = 6.4 x 105 !3! Insert your answer in decimal notation rounded to 2 decimal digits. Answer: Enter Value
- A chemistry graduate student is given 300. mL of a 1.60M pyridine (C H,N) solution. Pyridine is a weak base with K,=1.7 × 10 What mass of CH,NHC1 should the student dissolve in the CH,N solution to turn it into a buffer with pH = 5.16? You may assume that the volume of the solution doesn't change when the CH,NHCI is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.A buffer is made using 100.0 mL of 0.100 M CH3 CH2 COOH (propanoic acid) and 100.0 mL of 0.100 M NACH3 CH2 COO (sodium propanoate). A) Explain in your own words what will occur (at the molecular level) when an nitric acid is added to the buffer? What would be the effect on the pH? B) Explain in your own words what will occur when LIOH is added tot he buffer? What would be the effect on the [H+]?31. (a) Calculate the pH of a mixture containing 0.1 M propanoic acid (CH3CH₂COOH) and 0.050 M sodium propanoate (CH3CH₂COONa) (b) Determine the change in pH that occurs when 0.15 mol solid NaOH is added to 1.00 litre of the buffered solution. 32. (a) Calculate the pH of a buffer solution produced by adding 3.28 g of sodium ethanoate to 1 dm3 of 0.01 M of ethanoic acid (Ka = 1.84x 10-5 at 300K) (b) calculate the pH of this buffer if 10 cm3 of 0.1 M HCl are now added
