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Greeley [361]
3 years ago
13

At 25 °C, how many dissociated OH– ions are there in 1243 mL of an aqueous solution whose pH is 2.07?

Chemistry
1 answer:
coldgirl [10]3 years ago
3 0

<u>Answer:</u> The number of OH^- ions dissociated are 8.57\times 10^{11}

<u>Explanation:</u>

We are given:

pH = 2.07

Calculating the value of pOH by using equation, we get:

2.07+pOH=14\\\\pOH=14-2.07=11.93

To calculate hydroxide ion concentration, we use the equation to calculate pOH of the solution, which is:

pOH=-\log[OH^-]

We are given:

pOH = 11.93

Putting values in above equation, we get:

11.93=-\log[OH^-]

[OH^-]=10^{-11.93}=1.17\times 10^{-12}M

To calculate the number of moles for given molarity, we use the equation:

\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}

Molarity of solution = 1.17\times 10^{-12}M

Volume of solution = 1243 mL = 1.243 L  (Conversion factor: 1 L = 1000 mL)

Putting values in above equation, we get:

1.17\times 10^{-12}M=\frac{\text{Moles of }OH^-}{1.243L}\\\\\text{Moles of }OH^-=(1.17\times 10^{-12}mol/L\times 1.243L)=1.424\times 10^{-12}mol

According to mole concept:

1 mole of a compound contains 6.022\times 10^{23} number of particles

So, 1.424\times 10^{-12}mol number of OH^- will contain = (1.424\times 10^{-12}\times 6.022\times 10^{23})=8.57\times 10^{11} number of ions

Hence, the number of OH^- ions dissociated are 8.57\times 10^{11}

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