The pH of an aqueous solution of 0.0103 M hydrosulfuric acid, H2S (aq), is

Given, Molarity of H2S = 0.0103 M First acid dissociation constant of H2S = Ka1 = 1.0 x 10-7…

Answered: The pH of an aqueous solution of 0.0103…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 34P

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The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.
When carbon dioxide dissolves in water it reacts to produce carbonic acid, H2CO3(aq), which can ionize in two steps. H2CO3(aq)HCO3(aq)+H+(aq)Kc1=4.2107HCO3(aq)CO32(aq)+H+(aq)Kc2=4.81011 Calculate the equilibrium constant for the reaction H2CO3(aq)CO32(aq)+2H+(aq)
Use the appropriate tables to calculate H for (a) the reaction between MgC03(s) and a strong acid to give Mg2+(aq), CO2(g), and water. (b) the precipitation of iron(III) hydroxide from the reaction between iron(III) and hydroxide ions.
Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).
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?
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
The pH of an aqueous solution of 0.1690 M hydrosulfuric acid, H₂S (aq), is
What volume of 0.250 M HCl(aq) will completely react with 50.0 mL of 0.115 M NaOH(aq)? Write the balanced reaction and show the stoichiometry. Write the reaction of acetate ion in water. Predict the approximate pH of a solution with acetate ion present.
Find the pH of a 0.155 M HClO2(aq) solution
6. (i) Define pH in words. The strong acid HCl has a pH value of 1, use the following equation for a strong acid: aq HC1 aq à pH = -logo [H*] 10 Ht pH = aq + Cl and convert the following expression to deduce the hydrogen ion concentration: aq (ii) Use the above expression to deduce the pH of HCl (aq) given the concentration of the acid to be 4.5 mol/dm³
For each of the following entities Identify it as a strong or weak base. Select the correct arrow to show the changes that occur when the bases are placed in water. Select the approximate pH for each resulting solution. LIOH(aq) is classified as a base. The reaction equation with water utilizes which of the following arrows? Choice A Choice B 7 >>7 NaCH3CO0(aq) is classified as a se. The reaction equation with water would utilize which of the following arrows? Choice A Choice B < 50% CH3CO0 (aq) + H20(1) : CH3COOH(aq) + OH (aq) The approximate pH of the solution would be
Sodium hydrogen carbonate (NaHCO,, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI) , which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO, neutralizes excess HCl through this reaction: 圖 HCl(aq) + NaHCO3(aq) → NaCl(aq) + H,O(1) + CO,(g) The CO, gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 50. mL of a 0.089 M HCI solution. What mass of NaHCO, would he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits.

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