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Chapter 0: Q13P (page 1)

How many milliliters of 0.202MNaOHshould be added to 25.0 mlof 0.0233Msalicylic acid (2-hydroxybenzoic acid) to adjust the pHto 3.50?

Short Answer

Expert verified

The required volume ofNaOHis2.223mL

Step by step solution

01

Henderson-Hasselbalch equation

• The Henderson-Hasselbalch equation is a simplified formula that shows the connection between a solution's pH or pOH, pKa or pKb, and the ratio of concentrations of dissociated chemical species.

02

Determine the moles of salicylic acid

Calculate the moles of salicylic acid using the formula below: ηsalicylicacid=c×V

ηsalicylicacid=0.023M×25mL

ηsalicylicacid=0.5285mmo1

Consider the reaction:

localid="1663413505585" H2A+OH-⇌HA-+H2OH2A=0.5285-xHA-=x

03

Determine the required volume of NaOH

The Henderson-Hasselbach equation should be used next. pH=pKa+logHA-/H2A)3.50=2.972+logx0.5285-xx=0.4993mmol

Calculate the required volume of as follows V(NaOH)=n×cV(NaOH)=(0.4493mmol)×(0.202M)V(NaOH)=2.223mL

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Most popular questions from this chapter

A 10.231-g sample of window cleaner containing ammonia was diluted with 39.466 g of water. Then 4.373 g of a solution were titrated with 14.22 mL of 0.106 3 M HCl to reach a bromocresol green endpoint. Find the weight percent ofNH2(FM 17.031) in the cleaner.

In an experiment analogous to that in Figure 28-3, the sampling constant is found to be \({K_{\rm{s}}} = 20\;{\rm{g}}.\)

(a) What mass of sample is required for a \( \pm 2\% \)sampling standard deviation?

(b) How many samples of the size in part (a) are required to produce \(90\% \)confidence that the mean is known to within\(1.5\% \)?

What color do you expect to observe for the cresol purple indicator (Table 11-3) at the following pH values?

(a)1.0;(b)2.0;(c)3.0.

Calculate the formula mass ofCaSO4. What is the molarity of CaSO4in a solution containing 1.2gof CaSO4in a volume of 50 mL? How many grams of CaSO4are in 50 mLof 0.086MCaSO4?

Consider the following equilibria in aqueous solution:

(1)Ag++Cl-⇌AgCl(aq) K=2.0×103

(2)AgCl(aq)+Cl-⇌AgCl2-K=9.3×101

(3)AgCl(s)⇌Ag++Cl- K=1.8×10-10)

(a) Calculate the numerical value of the equilibrium constant for the reactionAgCl(s)⇌AgCl(aq).

(b) Calculate the concentration ofAgCl(aq)in equilibrium with excess undissolved solid AgCl.

(c) Find the numerical value ofKfor the reactionAgCl2-=AgCl(s)+Cl-
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