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Chapter 11: Q9P (page 259)

Find the equilibrium constant for the reaction of MES (Table9-2) withNaOH .

Short Answer

Expert verified

The equilibrium constant for the reaction of MES isK=5.4×107 .

Step by step solution

01

Define equilibrium constant.

When a chemical reaction is in equilibrium, the equilibrium constant gives information on the relationship between the reactants and products.The equilibrium constant is defined as the ratio of product concentration to reactant concentration, both elevated to their corresponding stoichiometric coefficients. It is given by the formula,

Kequ=kf/kb=CcDd/AaBb=Kc

where,

Kcis the equilibrium constant expressed in moles per liter.

02

Find the equilibrium constant.

The given reaction is a reaction between weak acid and a strong base.

HA+OH-⇌A-+H2O

Calculate the equilibrium constant using the formula,

K=1Kb1KwKa=KwKa=10-6.2710-14=5.4×107

Hence the equilibrium constant isK=5.4×107 .

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Most popular questions from this chapter

Consider the titration of100.0mlof 0.100MNaOHwith 1.00MHBr. Find the pH at the following volumes of acid added and make a graph of pH versusVa:Va=0,1,5,9,9,9,10,10.1 androle="math" localid="1654940659782" 12ml .

Why is it not practical to titrate an acid or base that is too weak or too dilute?

Titrating diprotic acid with strong base.

Prepare a family of graphs for the titration of 50.0 mL of 0.020 0 M H2A with 0.100 M NaOH. Consider the following cases: (a) pK1 = 4.00, pK2 =8.00; (b) pK1 = 4.00, pK2 = 6.00; (c) pK1 = 4.00, pK2 = 5.00

A50.0-mLsolution of 0.0319Mbenzylamine was titrated with0.0500MHCl.Calculate thepHat the following volumes of added acid: Va=0,12.0,12Ve,30.0,Ve, and 35.0mL.

Constant-boiling aqueous HCl can be used as a primary standard for acid-base titrations. When,20 wt% HCl (FM 36.461) is distilled, the composition of the distillate varies in a regular manner with the barometric pressure:

(a) Make a graph of the data in the table to find the weight percent of HCl collected at 746 Torr.

(b) What mass of distillate (weighed in air, using weights whose density is 8.0 g/mL) should be dissolved in 1.000 0 L to give 0.100 00 M HCl? The density of distillate over the whole range in the table is close to 1.096

g/mL. You will need this density to change the mass measured in vacuum to mass measured in air. See Section 2-3 for buoyancy corrections.
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