The balanced molecular equation for complete neutralization of H 2SO 4 by KOH in aqueous solution isH2SO4 (aq) + 2КОН (аq) — 2H20 (I) + К2S04 (s)BH2SO4 (aq) + 20H- (aq) → 2H2O (I) + SO42- (aq)(C) 2H+ (aq) + 20H- (aq) → 2H2O (I)DH2SO4 (aq) + 2KOH (aq) – 2H2O (I) + K2SO4 (aq)2H+ (aq) + 2KOH (aq) → 2H2O (I) + 2K+ (aq)E.

When an acid reacts with a base it produces salt and water. Such reactions are known as acid-base…

Answered: The balanced molecular equation for…

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions

Section: Chapter Questions

Problem 89GQ

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Vitamin C has the formula C6H8O6. Besides being an acid, it is a reducing agent. One method for determining the amount of vitamin C in a sample is to titrate it with a solution of bromine, Br2, an oxidizing agent. C6H8O6(aq) + Br2(aq) 2 HBr(aq) + C6H6O6(aq) A 1.00-g "chewable" vitamin C tablet requires 27.85 ml of 0.102 M Br2 for titration to the equivalence point. What is the mass of vitamin C in the tablet?
For an acid-base reaction, what is the reacting species (the ion or molecule that appears in the chemical equation) in the following bases? (a) barium hydroxide (b) trimethylamine (CH3)3N (c) aniline, C6H5NH2 (d) sodium hydroxide
A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?
A mountain lake that is 4.0 km × 6.0 km with an average depth of 75 m has an H+(aq) concentration of 1.3 × 10−6 M. Calculate the mass of calcium carbonate that would have to be added to the lake to change the H+(aq) concentration to 6.3 × 10−8 M. Assume that all the carbonate is converted to carbon dioxide, which bubbles out of the solution.
One half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total solution volume after mixing is 750. mL, what is the concentration of hydrochloric acid in the resulting solution? What is its pH?
87. What volume of 0.151 N NaOH is required to neutralize 24.2 mL of 0.125 N H2SO4? What volume of 0.151 N NaOH is required to neutralize 24.2 n1L of 0.125 M H2SO4?
A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. 1. If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!) 2.The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar. 3. Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.
North of Kingston you discover a hidden mountain and name it Mt. Kevinmanjaro, which weighs 1x1012 kg and is made entirely of CaCO3(s) (MW = 100 g/mol, Ksp = 3.3×10–9). Each year the mountain received approximately 1×106 L of rainfall, which flow from the mountain completely saturated with Ca2+(aq). How many years will it take to entirely dissolve Mt. Kevinmanjaro?
A. What is the pH of an aqueous solution with a hydrogen ion concentration of [H+]=4.9×10−7M? B. What is the hydroxide ion concentration, [OH−][OH−], in an aqueous solution with a hydrogen ion concentration of [H+]=4.9×10−7M? C. A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq)↽−−⇀H+(aq)+A−(aq) The equilibrium concentrations of the reactants and products are [HA]=0.270 M, [H+]=2.00×10−4 M, and [A−]=2.00 ×10−4 M. Calculate the ?a value for the acid HA.
Mg (OH)2 is used to neutralize hyperacidic condition of stomach as in the equation: Mg (OH)2+2HCl (aq) —> MgCl2 (aq)+ 2H2O (I) How many grams of HCl can be neutralized by 5.0g of Mg (OH)2
The Kc for the reaction 2A (aq) ⇌ 3 B (aq) is 0.085. What is Kc for the reaction 3 B (aq) ⇌ 2A (aq)?
Assume you titrated to the endpoint 0.10 moles of HA (weak, monoprotic acid) with a solution of sodium hydroxide, NaOH(aq), of unknown concentration. The initial volume of NaOH(aq) in the buret was 5.00 mL, and the final volume of NaOH(aq) in the buret was 45.00 mL. What is the concentration, in molarity, of the NaOH solution used?

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