The answer is: e. 12.70
pOH = -log[OH-] = -log[LiOH]
= -log(0.050) = 1.30
pH = 14 - pOH = 14 - 1.30 = 12.70
What is the pH of a 0.050 M LiOH solution? a. <1.0 b. 1.30 c. 3.00...
The PH of 0.0010 M of LiOH solution is? 3.00 13.00 4.00 11.00 2. The pKa values of acids A, B, C and D are 2.9, 4.1, 5.7 and 6.5, respectively. The weakest the acid is _____.
You have 10.5 g of LiOH and want to make a 1.30 M LiOH solution, what volume of solution can be made? 10. If you dilute 45 mL of a 3.6 M H2SO4 solution to a final volume of 175mL, what is the new concentration of H2SO4?
What is the ph of a 0.050 M triethylamine (C2H5) 3N solution? kB for triethylamine is 5.3 x 10^-4 5.32 2.31 1.30 8.68 or 11.69
The Ka of some acid, HA, at 25.0°C is 4.9 10-10. What is the pH of a 0.050 M aqueous solution of A? 1.0 x 10-3 O 9.9 x 10-12 11.00 3.00 O 2.5 x 10-11
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.
Find the pH of a 0.050 M HCl solution. What would be the final pH if 50.0 mL of the 0.050 M HCl solution was diluted to 250. mL?
Form 1 29. Determine the pH of a 0.741 M LiOH solution at 25°C. A) 0.130 B) 13.87 C) 0.741 D) 13.26 E) 1.18 30. What is the hydronium ion concentration of a 0.500 M acetic acid solu Ka = 1.8 x 10-5? The equation for the dissociation of acetic acid is: centration of a 0.500 M acetic acid solution with CH3CO2H(aq) + H2O(1) = H30+(aq) + CH3CO2"(aq) A) 3.0 x 10-2 M B) 4.2 x 10-2 M C) 3.0...
The Ka of some acid, HA, at 25.0 °C is 4.9 × 10-10. What is the pH of a 0.050 M aqueous solution of A-? 3.00 1.0 × 10-3 11.00 9.9 × 10-12 2.5 × 10-11
Calculate the pH of a solution prepared by dissolving 0.050 mol of benzoic acid (HA) and 0.50 mol of sodium benzoate (A-) in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.30 x 10-5 A. 5.20 B. 1.30 C. 7.00 D. 3.20 E. 4.20
6. 1.0 M Sulfuric Acid and 1.0 M NaOH a. What is the beginning pH? b. Write the complete balanced equation. c. Write complete ionic equation. d. List all precipitates that form. e. Write the net ionic equation. f. What is the pH of the solution after the reaction? Is it acidic, basic, or neutral?