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- Suppose that, instead of using NaOH, a base such as Ba(OH)2 had been used. What changes in the calculations would then have to be made to determine the molar concentrations of the base?The pOH of an aqueous solution of 0.392 M hydrocyanic acid, (K₁ (HCN) = 4.0 × 10−¹⁰) isUse the Referenc The pOH of an aqueous solution of 0.313 M acetylsalicylic acid (aspirin), HC9H¬O4, is
- The pH of an aqueous solution of 3.14×10-2 M ammonium chloride, NH4Cl (aq), isGiven 0.01 M solutions of each of the following acids, which solution would have the lowest pH? -117 Hypoiodous acid (HOI), K = 2.3 x 10 Hypobromous acid (HOBr), K = 2.5 x 10 Lactic acid (HC₂H₂O₂), K = 1.3 x 10 Chlorous acid (HClO₂), K = 1.1 x 10²Calculate the pH and the pOH of these solutions: (a) 0.0017 M NaOH pH = pOH = (b) 0.158 M HCl pH = pOH = (c) 0.0277 M HC6H5O (Ka = 1.3 x 10-10) pH = pOH =
- 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)The OH concentration in an aqueous solution at 25 °C is 3.1 x 103. What is [H*]?The OH concentration in an aqueous solution at 25 °C is 2.1 × 10 3. What is [H ]?
- The pH of an aqueous solution of formic acid (HCOOH) is 3.318. What is the initial molar concentration of HCOOH, if its acid ionization constant is Ka=1.78 × 10-4? Reaction: HCOOH (aq) ↔ HCOO- (aq) + H+ (aq).The pH of an aqueous solution of 0.532 M hydrofluoric acid, ( K₂ (HF) = 7.20 × 10-4) isThe pH of an aqueous solution of acetic acid (CH3COOH) is 2.0. What is the initial molar concentration of CH3COOH, if its acid ionization constant is Ka = 1.8×10–5?