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- At 50 °C, the ion-product constant for H2O has the valueKw = 5.48 x 10-14. (a) What is the pH of pure water at50 °C? (b) Based on the change in Kw with temperature,predict whether ΔH is positive, negative, or zero for theautoionization reaction of water:2 H2O(l) ⇌ H3O+(aq) + OH-(aq)You are given two glasses of water that have different temperatures. The temperature of the first glass is at 298 K, while the second glass has a temperature of 303 K. It has been determined that the Kw value for the second glass of water is 1.47 x 10-¹4. Which of the following statements is true? (a) The pH of the room temperature glass is higher, but both glasses have the same acidity. (b) The room temperature glass of water has a higher pH, and is more basic than the other glass of water. (c) Both glasses of water are neutral, so both will have a pH of 7.00. (d) The room temperature water has a lower pH, so is more acidic. (e) The warmer glass of water has a lower pH, and is more acidic than the other glass of water.Write the expression for K, and K, for the reaction PH;BCl,(s) = PH;(e) + BCl(g) 1.
- 1. the temperature for each solution is carried out at approximately 297 K where Kw = 1.00 x 10 ^-14 (a) 0.20 g of hydrogen chloride (HCl) is dissolved in water to make 4.5 L of solution. What is the pH of the resulting hydrochloric acid solution? (b) 0.70 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution ?A solution is prepared at 25 °C that is initially 0.36M in chlorous acid (HClO₂), a weak acid with K=1.1 × 10¯², and 0.29M in potassium chlorite (KC1O₂). -2 Calculate the pH of the solution. Round your answer to 2 decimal places. pH = 0 X ŚDetermine the pH of (a) A 0.10 M CH3COOH solution (ICE) (b) A solution that is 0.10 M CH3COOH and 0.10 M CH3COONa. Ka for CH3COOH = 1.8 X 10-5.
- 650.0 mL of HBr gas at 21.0 °C and 1025 mm Hg is absorbed completely into a solution that was created by mixing 7.147 g of Na2CO3 and 250.0 g of water. (a) What is the pH of the solution? (b) What is the freezing point of the solution?The pH of an aqueous solution of 0.400 M hydrocyanic acid, (Ka (HCN) = 4.00 × 10-10) isPropionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M HC3H5O2 and the pH of the solution? (b) What is the Kb value for the propionate ion, C3H5O2–? (c) Calculate the pH of 0.15 M solution of sodium propionate, NaC3H5O2. (d) Calculate the pH of solution that contains 0.12 M HC3H5O2 and 0.25 M NaC3H5O2.
- (7) Calculate the pH of each of the following solutions: (a) 0.1000M Propanoic acid( HC H O,,K=1.3x105) (b) 0.1000M sodium propanoate (Na C HỎ) (c) 0.1000M HC₂H₂O, and 0.1000M Nа С¸¸0₂ 3 5 52 (d) After 0.020 mol of HCl is added to 1.00 L solution of (a) and (b) above. (e) After 0.020 mol of NaOH is added to 1.00 L solution of (a) and (b) above.Discuss the justification for this statement: “Although one does not normally regard NH+4 as an acid, it is actually only slightly weaker as an acid than hydrocyanic acid, HCN, in aqueous solution.”7 (a) Describe what happens when each of the following molecules is separately dissolved in water and illustrate with an equation in each case: (i) ethanoic acid (CH₂COOH) (ii) ammonia (NH3) (b) Identify the conjugate acids and bases in the substances mentioned in question 7(a) above. (c) Explain the difference between: (i) a strong acid and weak acid and (ii) a strong base and a weak base