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A: Below attached file showing the details answer. All the best.
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What is the pH at 25degrees Celsius of a saturated solution of silver hydroxide? (Ksp value for silver hydroxide is 2.0 x 10^-8)
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- Like all equilibrium constants, the value of KwKw depends on temperature. At body temperature (37 ∘C∘C), Kw=2.4×10−14Kw=2.4×10−14. What is [H3O+][H3O+] in pure water at body temperature?What is the pH of a saturated solution of silver hydroxide, given Ksp = 1.57×10-8?The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. 1. what is the pH when the volume of base added equals half the volume of the equivalence point? 2. what is the pH of the titration when 20.00 mL of base have been added? 3. what is the pH of the titration when 30.00 mL of base have been added?
- The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. a) Sketch the pH vs volume of added base titration curve for this reaction. pH vertically, volume of base horizontally. Label your axes with correct pH and volumes. (Attach more space, if needed) b) what is the pH at the beginning of the titration, Vbase = 0.00 mL ? c) what is the volume of the base needed to reach the equivalence point ? (label the equiv. point) d) what is the pH at the equivalence point?e) what is the pH of the titration when 5.00 mL of base have been added ? f) what is the pH when the volume of base added equals half the volume of the equivalence point? g) what is the pH of the titration when 20.00 mL of base have been added? h) what is the pH of the titration…The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. A. What is the pH at the beginning of the titration, Vbase = 0.00 mL? B. What is the pH at the equivalence point? C. What is the pH of the titration when 5.00 mL of base have been added? D. What is the pH when the volume of base added equals half the volume of the equivalence point? E. What is the pH of the titration when 20.00 mL of base have been added? F. What is the pH of the titration when 30.00 mL of base have been added?Suppose that the solubility of Ca(OH)2 in water is 0.3g/0.1L. What is the pH of an aqeous saturated solution of Ca(OH)2?
- What is the pH of a saturated solution of Fe(OH)₂? Ksp pH = X = 4.87 x 10 17 Be sure your answer has the correct number of significant digits.The solubility product of nickel(II) hydroxide, Ni(OH)2, at 25°C is Ksp = 1.6 × 10-16.(a) Calculate the molar solubility of Ni(OH)2 in pure water at 25°C.(b) Calculate the molar solubility of Ni(OH)2 in 0.100 M NaOH.Ammonium hexachloroplatinate(IV), (NH4)2(PtCl6), is one of the few sparingly soluble ammonium salts. Its Ksp at 20°C is 5.6 × 10-6. Compute its solubility in grams per liter of solution.
- Benzoic acid, C6H5COOH, dissociates in water as shown in the equation below. A 40.0 mL sample of an aqueous solution of benzoic acid with a concentration of 0.50 M is titrated using standardized 0.25 M NaOH. C6H5COOH(s) ⇄ C6H5COO–(aq) + H+(aq) Ka = 6.46 x 10–5 a.Calculate the pH of the solution after the following amounts of NaOH have been added… 0 mL 10 mL 85 mL b. State whether the solution at the equivalence point of the titration is acidic, basic, or neutral. Explain your reasoning. c. How many mL of 0.25 M NaOH need to be added in order to make the ideal buffer solution?Calculate the molar solubility of lead(II) iodide in water at 25°C, given that its Ksp = 7.1 × 10−9 .A student titrates 20.0 mL of 1.0 M NaOH with 2.0 M formic acid, HCOOH (K, = 1.8 x 104). Hypochlorous acid is an unstable compound and one of the decomposition products is chlorine gas, Cl2. The composition of the acid lowers its concentration over time. What effect will the decomposition of one-fourth of the acid have on the agreement between the endpoint of the titration and the equivalence point during a titration with standard sodium hydroxide? It is impossible to determine The endpoint would be before the ideal equivalence point The endpoint would be after the ideal equivalence point The endpoint will rema eerthe ideal egvaleacepolnt
