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Chapter 6: Q3TY (page 132)

Use Table 6-1 to find the [H+]in water at 100°Cand at0°C.

Short Answer

Expert verified

H+in the water at 100°C and at 0°Care found to be 7.4×10-7 and ,3.4×10-8 respectively.

Step by step solution

01

Define the formula for finding Kb.

The value of can be calculated as:

Kb=[BH+][OH][B]

Where Kbis called the base dissociation constant.

02

Step 2: Calculate the Kw.

Given:

At100°C,Kw=5.43×10-13

At0°CKw=1.15×10-15

Kw=[H+][OH-]

H+in the water at100°C

Kw=5.43×10-14=[H+][OH-]=[x][x]=[x]2x=5.43×10-14=7.4×10-7

At 0°C

Kw=1.15×10-15=[H+][OH-]=[x][x]=[x]2x=1.15×10-15=3.4×10-8

Using temperature dependent of Kwavalues H+in the water.

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Most popular questions from this chapter

Explain why hydrated metal ions such as(H2O)Fe3+ hydrolyze to give H+ , but hydrated anions such as(H2O)6CI- do not hydrolyze to give H+.

Reaction 6-8 is allowed to come to equilibrium in a solution initially containing0.0100MBrO3-,0.0100MCr3+ and 1.00MH+. To find the concentrations at equilibrium, we construct the table at the bottom of the page showing initial and final concentrations. We use the stoichiometry coefficients of the reaction to say that if xmolof Br- are created, then we must also make x mol of Cr2O72- and 8x mol of H+. To produce x mol of Br-, we must have consumed x mol of Br-O3- and 2x mol of Cr3+.

(a) Write the equilibrium constant expression that you would use to solve for x to find the concentrations at equilibrium. Do not try to solve the equation.

(b) Because K=1×1011, we suppose that the reaction will go nearly "to completion." That is, we expect both the concentration of Br-and Cr2O72-to be close to 0.00500M an equilibrium. (Why?) That is, x≈0.00500M. With this value of x,[H+]=1.00+8x=1.04Mand [BrO3-]=0.0100-x=0.0050M. However, we cannot say [Cr3+]=0.0100-2x=0, because there must be some small concentration of Cr3+at equilibrium. Write [Cr3+]for the concentration of Cr3+and solve for [Cr3+]. The limiting reagent in this example is Cr3+. The reaction uses up before consuming BrO3-.

For the reaction 2A(g)+B(aq)+3C(l)⇌D(s)+3E(g), the concentrations at equilibrium are found to be

A:2.8×103Pa

B: 1.2×10-2M

C:12.8M

D: 16.5M

E:3.6×104Torr

Find the numerical value of the equilibrium constant that would appear in a conventional table of equilibrium constants.

A solution contains 0.0500MCa2+and 0.0300MAg+. Can 99%of Ca2+be precipitated by sulphate without precipitatingAg+? What will be the concentration ofCa2+whenAg2SO4begins to precipitate?

Write the autoprotolysis reaction ofH2SO4.
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