QUESTION 1 A weak acid, HA, has an equilibrium constant, Ka, of 0.0000007624. If a soluiton is made of 0.922M HA, what is the expected pH of the solution?
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- The weak base, CIO (hypochlorite ion), is used in the form of NaCIO as a disinfectant in swimming pools and water treatment plants. What are the concentrations of HCIO and OH and the pH of a 0.015 M solution of NaCIO?What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.Calculate [OH-] and pH in a solution in which the hydrogen sulfite ion, HSO3-, is 0.429 M and the sulfite ion is (a) 0.0249 M (b) 0.247 M (c) 0.504 M (d) 0.811 M (e) 1.223 M
- Differentiate between the terms strength and concentration as they apply to acids and bases. When is HCl strong? Weak? Concentrated? Dilute? Answer the same questions for ammonia. Is the conjugate base of a weak acid a strong base?Consider the process H2O H+(aq)+OH(aq)H=55.8kJ (a) Will the pH of pure water at body temperature (37C) be 7.0? (b) If not, calculate the pH of pure water at 37C.A student prepares 455 mL of a KOH solution, but neglects to write down the mass of KOH added. His TA suggests that he take the pH of the solution. The pH is 13.33. How many grams of KOH were added?
- How many significant figures are there in the following numbers: 10.78, 6.78, 0.78? If these were pH values, to how many significant figures can you express the [H+]? Explain any discrepancies between your answers to the two questions.You are asked to calculate the H+ concentration in a solution of NaOH(aq). Because sodium hydroxide is a base, can we say there is no H+. since having H+ would imply that the solution is acidic?Determine the pH of the solution resulting from mixing a solution of 153 mL of CH₂BrCOOH (Ka = 1.26e - 03) at a 1.540 M concentration, with 136 mL of a 1.380 M solution of KOH? O (a) 0.317 (b) 3.492 (c) 2.492 (d) 1.746 O (e) 2.900
- Human blood has pH=7.4 . Therefore, its (a) [OH-] =3.28x10-8(M) (b) [H+] =3.28x10-8(M) (c) [H+] =3.28x10-7(M) (d) [H+] = 10-7.4 (M) (e) pOH=8.635. Calculate the pH of a solution that is 0.15 M in formic acid (HCOOH) and 0.20 M in sodium formate (HCOONa). The K₂ of formic acid is K₂ = 1.8×10-4. (A) 9.21 (B) 3.87 (C) 4.53 (D) 7.00 (E) 1.15Calculate the pH of a solution containing 0.20 M CH3COOH and 0.30 M CH;COONA. [Ka CH3COOH = 1.8 x 1051 8. (a) 4.9 (b) Calculate the pH of the 0.20 M CH3COOH solution if there is no salt present. [Ka CH3COOH = 1.8×10-°] 2.7 (c) Explain the change in pH the solution in (a) when i. a small amount of strong acid is added. ii. a small amount of strong base is added.