Consider a 1.0-L solution that is 0.480 M HCOOH and 0.83 M NaHCOO at 25 °C. What is the pH of this solution before and after 0.018 moles of HNO3 have been added? Ka of HCOOH is 1.7E-4
initial pH: 4.01, final pH: 3.56.
initial pH: 4.01, final pH: 3.98.
initial pH: 3.53, final pH: 4.03.
initial pH: 3.53, final pH: 3.51.
initial pH: 3.77, final pH: 4.03.
Consider a 1.0-L solution that is 0.480 M HCOOH and 0.83 M NaHCOO at 25 °C....
Consider a 1.0-L solution that is 0.480 M C5H5N and 0.17 M C5H5NHCl at 25 °C. What is the pH of this solution before and after 0.012 moles of HI have been added? Kb of C5H5N is 1.7E-9 a-initial pH: 4.78, final pH: 5.72 .b- initial pH: 5.68, final pH: 5.64 .c- initial pH: 5.68, final pH: 5.74. d-initial pH: 5.23, final pH: 4.82. e-initial pH: 5.68, final pH: 4.82
Consider a 1.0-L solution that is 0.830 M HNO2 and 0.37 M NaNO2 at 25 °C. What is the pH of this solution before and after 0.011 moles of LiOH have been added? Ka of HNO2 is 4.5×10-4. initial pH: 3.7, final pH: 2.98. initial pH: 3.35, final pH: 2.98. initial pH: 3.0, final pH: 3.68. initial pH: 3.7, final pH: 3.72. initial pH: 3.0, final pH: 3.01.
23. A 1.0 L buffer solution is prepared with 0.25 M formic acid (HCOOH) and 0.50 M sodium formate (HCOONa). HCOOH(aq) + H2O(aq) – HCOO (aq) + H30+(aq) pKa = 3.74 What is the pH of this buffer solution? (A) 3.74 (B) 4.04 (C) 4.50 (D) 4.20
2. A formic acid buffer containing 0.50 M HCOOH and 0.50 M HCOONa has a pH of 3.77. What will the pH be after 0.010 mol of NaOH has been added to 100.0 mL of the buffer? A) 3.67 B) 3.78 C) 3.81 D) 3.85 E) 3.95 A buffer is prepared by adding 1.00 L of 1.0 M HCl to 750 mL of 1.5 M Nalcoo. What is the pH of this buffer? Ka = 1.7 * 104 A) 2.87...
You have 2.50 L of a 0.450 M HCOOH and 0.550 M HCOONa buffer solution. (Ka for HCOOH is 1.8x10^-4) a) Calculate the pH of the buffer solution. b) Determine the pH of the buffer solution after the addition of 0.150 mol of NaOH (assume no change in volume).
What quantity (moles) of NaOH must be added to 1.0 L of 1.8 M HC2H3O2 to produce a solution buffered at pH = 4.00? Ka = 1.8×10-5
A 1.0 L solution initially contains 0.3 M CH3COOH. Approximate the number of moles of CH3COOH and CH3COO− in the solution after 0.1 mol of solid NaOH is added, and calculate the pH of the resulting solution. Ka of CH3COOH is 1.8 ×10−5. 1) The number of moles of CH3COOH present is [ Select ] ["0.2", "0.3", "0.1"] mol. 2) The number of...
23) What is the pH of a solution prepared by mixing: 0.20 moles of acetic acid 0.40 moles of sodium acetate 0.10 moles of sodium hydroxide in 1.0 L of solution a) 4.74 b) 4.14 5.34 d) 13.00 e) None of the above 24) Barbituric acid (Ka = 9.8 X 10-5) is titrated with 0.200 M NaOH. What is the initial pH of 20.0 mL of 0.100 barbituric acida) 2.50 b) 4.01 c) 8.35 d) 7.00 e) None of the above 25) What is the pH in...
A buffer solution contains 1.0 M HF and 1.0 M NaF. The ka for HF is 7.2x10-5. 0.10 moles of HCl are added to 1 liter of the buffer. The pH of the resulting solution is a) 4.05 b) 4.14 c) 4.23 d) 4.74
1.0 L of a 1.2 M solution of formic acid (Ka=1.8x10-4) was prepared. What is the pH of this solution? 1.8328 You are correct. Your receipt no. is 162-1608 Previous Tries Enough potassium formate was added to achieve a final potassium formate concentration of 1.7 M (assume the volume does not change). What is the pH of this new solution? 3.8960 You are correct. ceipt no. is 162-6598 Previous Tries 10 mL of 10 M NaOH is added to the...