Question 6 If the hydroxide ion concentration of a 0.109 M NH, solution is 0.0014 M. what is the ionization constant for ammonium? NHy(80)+ H2O(l) +) NHã (0) + OH() Ki-14×10³ harkintage Ki-1.8 -105 Ki-1.8 - 10. K-18-104 -13-10² Cheqq RE
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- Which of the following salts would give you the lowest concentration of sulfate ions in solution if you placed 1 mole of the salt in a liter of water? Question 6 options: A) BaSO4 Ksp= 1.1 x 10-10 B) CaSO4 Ksp= 2.4 x 10-5 C) SrSO4 Ksp= 2.8 x 10-7 D) PbSO4 Ksp= 1.8 x 10-8What is the pH of a solution when 82.5 mL of a 0.1M HCN solution (ka = 6.2 x 10 -10) is titrated with 41 mL of a 0.085M NaOH solution? Question 6 What is the pH of an aqueous solution containing 53.5mL of a 0.1 HNO2 solution (ka = 4.5 x 10 -4) and 69.4mL of a 0.11M KNO2 after 10.0mL of a 0.075M HNO3 solution is added? Question 7 What is the pH of a 75.0mL of a 0.1M pyridine (C5H5N) solution (kb = 1.7 x 10 -9) when 100mL of a 0.075M HI (aq) solution is added?NH4F is a salt made from a weak base and a weak acid. The following questions are related to a 0.250 M NH4F (aq) solution at 25 degrees C. The Ka for HF (aq) is 6.8 ×10-4 and Kb for NH3 (aq) is 1.8 × 10-5. (a) What is the equation for the overall hydrolysis of NH4F (aq)? (b) What is the pH of this solution? (c) What is the equilibrium concentration of NH3?
- Question one .) A 0.325 g tablet of aspirin (acetylsalicylic acid, HAsc, C9H8O4) is dissolved in 0.500 L of water. The acid ionization constant Kafor HAsc is 3.3 x 10–4. What is the pH of this solution? Question 2.) 0.0015 M solution of a weak base has a pH of 9.84. Calculate Kb.1: If Kb for NX3 is 7.0×10−6, what is the pOH of a 0.175 M aqueous solution of NX3? 2: If Kb for NX3 is 7.0×10−6, what is the percent ionization of a 0.325 M aqueous solution of NX3? 3: If Kb for NX3 is 7.0×10−6 , what is the the pKa for the following reaction? HNX3+(aq)+H2O(l)⇌NX3(aq)+H3O+(aq)Question 20 Calculate the percentage of pyridine (C5H5N) that forms pyridinium ion, C5H6N+, in a 0.89 M aqueous solution of pyridine (Kb = 1.7
- Milk of Magnesia is not very soluble in water. Mg(OH)2 ⇌Mg2+(aq) + 2OH-(aq), Ksp =1.8 x10 -11 at 25°C A saturated solution has a pH of 10.5 and the Mg2+ concentration is 1.7 x 10-4 M. If the pH is changed to 9.0 how does this affect the Mg2+ concentration? Question 2 options: a) [Mg2+] = 1.6x10-4 M b) [Mg2+] = 1.0x10-5 M c) [Mg2+] = 1.8x101 M d) [Mg2+] = 1.7x10-4 MKb for NH3 is 1.8 × 10-5. What is the pOH of a 0.20 M aqueous solution of NH4Cl at 25.0 °C? A) 2.72 B) 11.28 C) 9.02 D) 4.98 E) 11.23Question 3:What is the pH of a 0.119 M HA acid solution if the ionization constant (KA) of this acid is 0.24 .
- The propionate ion, CH3CH2COO–, reacts with water as a weak base: CH3CH2COO–, (aq) + H2O(l) ⇄ CH3CH2COOH(aq) + OH–(aq), with K = 7.4 x 10-10 at 25°C. If sodium propionate were dissolved in water to make a 0.60 M solution, what would be the resulting concentration of OH–? (no scientific notation)Question 4 4.1 Calculate the acid ionization for Ka for propionic acid, HC3H5O2. The pH of a 0.012 M aqueous solution is 3.40. 4.2 Boric acid, B(OH)3, is used as a mild antiseptic. What is the pH of a solution of a 0.025 M aqueous solution of boric acid? What is the degree of ionization of boric acid? The hydrogen ion arises principally from the reaction: The equilibrium constant for this reaction is 5.9 .Question: 1 .HA is a weak acid. Its ionization constant, Ka, is 1.3 x 10-13. Calculate the pH of an aqueous solution where the initial concentration of NaA is 0.050 M. 2 . Place 0.112 mol of a weak acid, HA, in enough water to make 1.00 L of solution. The final pH of this solution is 1.29. Calculate the ionization constant, Ka, of HA. 3 . Place 0.648 mol of a weak acid, HA, and 13.1 g of NaOH in enough water to produce 1.00 L of solution. The final pH of this solution is 4.76. Calculate the ionization constant, Ka, of HA. Please complete answers than rating helpful other wise un helpful