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![In an aqueous solution at 25 °C, if [H₂O+] = 5.6 × 10 M, then [OH] is:](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F99091e55-84ac-4709-a57b-335d8cd227fa%2Fab9da2c1-11a5-4639-b35f-14482b8cdb7b%2F58skofc_processed.png&w=3840&q=75)
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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?Use the Referenc The pOH of an aqueous solution of 0.313 M acetylsalicylic acid (aspirin), HC9H¬O4, isThe pOH of an aqueous solution of 0.392 M hydrocyanic acid, (K₁ (HCN) = 4.0 × 10−¹⁰) is
- The pH of an aqueous solution of 3.14×10-2 M ammonium chloride, NH4Cl (aq), isAt 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)Calculate 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 =
- Given 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 10²The 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) isPlease answer these questions on your Page 8 (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 7.7 x 10-¹2. What is the pH of a 0.011 M solution of A-(aq)? The temperature is 25°C. (b) For the reaction A(g) A(1), the equilibrium constant is 0.666 at 25.0°C and 0.111 at 75.0°C. Making the approximation that the entropy and enthalpy changes of this reaction do not change with temperature, at what temperature will the equilibrium constant be equal to 0.777?
