9. (2pts total) a. A solution of a weak acid with concen its K, value. with...
9 & 10 BUIL OTO 10-4.26 = 5.49x105 pOH - 4.26 9. (ps total) a. A solution of a weak acid with concentration its K, value. 0.11 M. is 8.8 % ionized. Calculate K =_ b. Calculate the K, value of a 0.060 M solution of a monoprotic acid with [H'] = 2.7 x 10-2 M. K. =
please help with numbers 7, 8 and 9 showing work 7. If H.PO, has K. -6.83 x 10', and H.CO, has K, -5.8 x 10", which is the weaker acid? Circle your answer and explain how you know. (pt) 8. For a solution with pH = 9.74, calculate the following: 3ps) [OH) = pOH - 9. (pes total) a. A solution of a weak acid with concentration - 0.11 M. is 8.8 % ionized. Calculate its K, value b. Calculate...
7. If H,PO, has K, -6.83 x 10, and Hco, has K,-5.8x 10", which is the weaker acid? Circle your answer and explain how you know. (Ipt 8. For a solution with pH 9.74, calculate the following: (3pa) [H'] [OH] pOH- 9. (2pas total) a. A solution of a weak acid with concentration 0.11 M. is 8.8 % ionized. Calculate its K, value. K, b. Calculate the K, value of a 0.060 M solution of a monoprotic acid with [H']...
K.- b. Calculate the K, value of a 0.060 M solution of a monoprotic acid with (H) - 27 x 10" M. K,
please help me with these questions! At a concentration of 1 M, the weak acid HNO, is 2% ionized, and the pH of the solution is 1.7. What happens when KNO,() is dissolved into the solution? The extent of HNO, ionization The concentration of H+ The pH If a buffer solution is 0.260 M in a weak acid (K, = 6.0 x 10 ) and 0.500 M in its conjugate base, what is the pH? A 0.194 g sample of...
Question HA is a weak acid. Its ionization constant, K, is 3.0 x 10) Calculate the pH of an aqueous solution with an initial NaA concentration of 0.060 M. Question 2 We place 0.150 mol of a weak acid, HA, in enough water to produce 100L of solution. The final pH of the solution is 1.18. Calculate the ionization contant, K., HA. Question We place 0.607 mol of a weak acid, HA, and 13.9 g of NaOH in enough water...
7. Lactic acid (CSH COOH) is a weak monoprotic acid whose K, value is 1.4x10". Its salt potassium lactate is added to food products as a preservative and to inhibit growth of bacteria. What is the pH of a solution whose molar concentration of potassium lactate (CSHCOO-K) is 0.290 M? Caution! This problem does not say that lactic acid is dissolved in water, it is potassium lactate that is added to the water.
A. What is the pH of an aqueous solution with a hydrogen ion concentration of H] = 8.8 x 10-'M? pH = B. What is the hydroxide ion concentration, (OH), in an aqueous solution with a hydrogen ion concentration of [H+] = 8.8 x 10-'M? [OH-] = C. A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) =H(aq) + (aq) The equilibrium concentrations of the reactants and products are [HA] = 0.300 M, H+] = 4.00...
28. An initially 1.8 M aqueous solution of a weak monoprotic acid has a total ion concentration has a total ion concentration of 8.45 x 10-3 M when equilibrium is established. What is the acid-ionization constant, K of the weak acid? (assume n a. 3.3 x 10-2 b. 6.8 x 10-2 c. 1 x 10-5 d. 7.1 x 10-5 e. 2.7 x 100
3) Hypobromous acid (HOBr) is a weak monoprotic acid, with K. = 2.1 x 10-9 a) What is the value for pH for a 0.0424 M aqueous solution of hypobromous acid? [12 points) I b) 0.0100 moles of NaOH, a strong soluble base, is added to 1.000 L of the above solution of hypobromous acid. What will be the pH for this new solution? [15 points]