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Chapter 8: QDE (page 182)

Using activities, calculate the pH and concentration of H+in 0.050MLiBr at25°C.

Short Answer

Expert verified

The pH of the given solution is 6.99

Step by step solution

01

Define the formula for PH calculation.

The pH of a solution can be calculated as,

pH=-logAH+=-log[H+]γH+

where,

AH+ - activity of hydrogne ion

γH+ - activity coefficient of hydrogne ion.

02

Calculate the PH form the activity.

Given

0.050MLiBr at 25°C

At an ionic strength role="math" localid="1654765585845" μof andγOH=0.81.

role="math" localid="1654765776290" H+γH+OH-γOH=x0.86x0.81=1.0×10-14x=1.2×10-7M.

The concentration of H+ion is1.2×10-7M

Calculate the pH by using the concentration of H+ion

pH=-log1.2×10-70.86=6.99

Thus, theof the given solution is 6.99 .

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Most popular questions from this chapter

Explain why the solubility of an ionic compound increases as

the ionic strength of the solution increases (at least up to ,0.5 M ).

Solubility with Activity: Find the concentration of the major species in a saturated aqueous solution of LiF. Consider these reactions:

LiFs֏Li++F-Ksp=Li+γLi+F-γF-LiFs֏LiFaqKionpair=LiFaqγLiFaqF-+H2O֏HF+OH-Kb=KwKaforHFH2O֏KwH++OH-Kw=H+γH+OH-γOH-

  1. Look up the equilibrium constants in the appendixes and write their pK values. The ion pair reaction is the sum of localid="1654945209684" LiFs֏Li++F-from the Appendix FandLi+֏LiFaqfrom Appendix J. write the equilibrium constant expressions and the charge and mass balance.
  2. Create a spreadsheet that uses activities to find the concentration of all species and the ionic strength. Use pH and pOH as independent variables to estimate. It does not work to choose pH and pLi because their concentration fixes that of the other through the relation Ksp=Li+γLi+F-γF-

(a) Following the example of Mg(OH)2 in Section 8-5, write the equations needed to find the solubility of Ca(OH)2. Include activity coefficients where appropriate. Look up the equilibrium constants in Appendixes F and I.

(b) Suppose that the size of CaOH+= Ca(H2O)5(OH)+ is 500 pm. Including activity coefficients, compute the concentrations of all species, the fraction of hydrolysis (= [CaOH+]/{[Ca2+] + [CaOH+]}), and the solubility of Ca(OH)2 in g/L. The Handbook of Chemistry and Physics lists the solubility of Ca(OH)2 as 1.85 g/L at 00C and 0.77 g/L at 1000C

Using activities, calculate the pH of a solution containing 0.010 M NaOH plus 0.012 0 M LiNO3 . What would be the pH if you neglected activities?

Including activity coefficient, find the concentration of Ba2+in 0.100M(CH3)4NIO3solution saturated with Ba(IO3)2.
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