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4. An aqueous buffer solution if made from 150.0 mL of a 1.50 M HCN solution...
Calculate the following: a. The pH of a 500.0 mL buffer solution containing 0.75 M HCN (Ka = 6.2 x 10^-10) and 0.55 M NaCN b. The pH of the above buffer after the addition of 100.0 mL of 1.0 M NaOH. c. The pH of the buffer if 100.0 mL of 1.0 M HCl was added to the solution in part a.
Calculate the volumes of 0.200 M hydrocyanic acid, HCN (Ka = 4.9 x 10–10) solution, and 0.200 M of sodium cyanide, NaCN, solution needed to prepare 100.0 mL buffer solution with pH = 9.5
37. You have 500.0 mL of a buffer solution that is 0.30 M HF and 0.50 M KF. Ka for HF is 7.1 x 10-4 a) Calculate the pH of the buffer. b) Calculate the pH of the buffer after adding 0.020 moles of HCI. c) Calculate the pH of the buffer after adding 0.030 moles KOH. - -Loel.
22. A 100.0-ml buffer solution is 0.175 M in HCIO and 0.150 M in Nacio. a. What is the initial pH of this solution? b. What is the pH after addition of 150.0 mg of HBr?! c. What is the pH after addition of 85.0 mg of NaOH?
18. You are asked to prepare a pH = 8.60 buffer starting from 500 mL of 0.10 M solution of hydrocyanic acid, HCN, and excess sodium cyanide, NACN. (Ka for HCN = 4.9 x 10-10) a) What is the pH of the hydrocyanic acid solution prior to adding NACN? b) How many grams of NaCN should be added to prepare the buffer solution?
D. Buffers 1. A buffer solution was made by dissolving 10.0 grams of sodium acetate in 200.0 mL of 1.50 M acetic acid. Assuming the change in volume when the sodium acetate is added is not significant, estimate the pH of the acetic acid/sodium acetate buffer solution. The K, for acetic acid is 1.8 x 105. 2. Calculate the pH of a buffer solution that initially consists of 0.0400 moles of ammonia and 0.0250 moles of ammonium ion, after 20.0...
1. A buffer solution is 0.313 M in HCN and 0.220 M in NaCN . If Ka for HCN is 4.0×10-10, what is the pH of this buffer solution? 2. A buffer solution is 0.473 M in H2C204 and 0.366 M in KHC2O4 . If Ka1 for H2C2O4 is 5.9*10^-2, what is the pH of this buffer solution? 3. A buffer solution is 0.392 M in NaHC2O4 and 0.329M in NaC2O4 . If Ka for HC2O4- is 6.4*10^-5, what is...
Which of the following could you add to 100.0 mL of 1.0 M HCN to make a suitable buffer system? (There may be more than one correct answer.) 100.0 mL of 0.050 M NaCN, 100.0 mL of 0.20 M NaCN, 100.0 mL of 1.0 M NaCN, 100.0 mL of 0.050 M NaCl, 100.0 mL of 0.20 M NaCl, 100.0 mL of 0.050 M HCN, 100.0 mL of 0.20 M HCN, 100.0 mL of 1.0 M HCN, 50.0 mL of 1.0...
Please explain how to get the net ionic equations. A buffer solution is made that is 0.464 M in HCN and 0.464 M in KCN. If Ka for HCN is 4.00 x 10-10, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.115 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) A buffer solution is made...
34/35 A buffer solution is made that is 0.411 M in HClO and 0.411 M in Nacio. If K, for HCIO is 3.50 x 10-8, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.122 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) A buffer solution is made that is 0.365 M in HCN and 0.365...