What is the pH of a 0.055 M solution of sodium cyanide? The Ka value for hydrocyanic acid is 6.2 x 10-10.
Select one:
a. 10.08
b. 8.77
c. 10.97
d. 5.23
e. 3.03
What is the pH of a mixture containing 0.33 M HNO2 and 0.20 M NaNO2? (Ka for HNO2 = 4.5 x 10-4)
Select one:
a. 7.8
b. 3.57
c. 3.13
d. 1.22
e. 3.35
What is the molar solubility of Zn2+ in a solution that is buffered at a pH of 4.00? The Ksp for Zn(OH)2 is 3 x 10-17.
Select one:
a. 6 x 10-23 mol/L
b. 7 x 10-4 mol/L
c. 3000 mol/L
d. 3 x 10-7 mol/L
e. 3 x 10-17 mol/L
What is the pH of a 0.055 M solution of sodium cyanide? The Ka value for...
What is the pH of a solution prepared to 0.040 M NaNO2. Ka HNO2 = 7.1 x 10-4
A buffer solution contains 0.58 mol of hydrocyanic acid (HCN) and 0.68 mol of sodium cyanide (NaCN) in 3.00 L. The Ka of hydrocyanic acid (HCN) is Ka = 4.9e-10. (a) What is the pH of this buffer? pH = (b) What is the pH of the buffer after the addition of 0.46 mol of NaOH? (assume no volume change) pH = (c) What is the pH of the original buffer after the addition of 0.23 mol of HI? (assume...
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.
A buffer solution contains 0.64 mol of hydrocyanic acid (HCN) and 0.59 mol of sodium cyanide (NaCN) in 5.10 L. The Ka of hydrocyanic acid (HCN) is Ka = 4.9e-10. (a) What is the pH of this buffer? pH = 9.345 (b) What is the pH of the buffer after the addition of 0.44 mol of NaOH? (assume no volume change) pH = (c) What is the pH of the original buffer after the addition of 0.25 mol of HI?...
What is the pH of aqueous 0.10 M HNO2? Ka(HNO2) = 4.5 x 10-4 a. 1.67 b. 3.35 c 1.00 d. 4.35 e. 2.17
A buffer solution contains 2.15 M hydrocyanic acid and 0.60 M cyanide ion. What is the pH of the buffer? (The Ka of hydrocyanic acid is 6.2x10-10.) 9.76
Calculate the pH of a 0.263 M solution of NaNO2. The ionization constant, Ka, for the acid, HNO2, is 4.60×10−4. pH=
11. Calculate the pH of a solution of 0.10 M hydrogen cyanide HON? (Ka = 4.9 x 10-10) E. 9.31 F. 5.15 G. 4.16 H. 1.00
Calculate the pH of a solution that is prepared by dissolving 0.470 mol of hydrocyanic acid (HCN, Ka = 6.17×10-10) and 0.180 mol of nitrous acid (HNO2, Ka = 4.60×10-4) in water and diluting to 2.30 L. Also, calculate the equilibrium concentrations of HCN, CN-, HNO2, and NO2-. Do not make an approximation unless the initial acid concentration is greater than 1000 × Ka. (Hint: The pH will be determined by the stronger acid of this pair.) pH = [HCN]...
Calculate the pH of a solution of 0.10 M hydrogen cyanide HCN? (Ka = 4.9 x 10-10) The answer is 5.15 please explain.