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3 years ago

Calculate the pH of a solution on mixing 0.1 M (50 mL) Ch3cooh and 0.1M(50 mL) NaohKa= 0.00005

Chemistry

1 answer:

Margaret [11]3 years ago

6 0

Answer:

here

Explanation:

Ka=Cx^2/1-x

Ka =1.8 x 10^-5

C = 0.1

If we consider x is negligible ie., x~0

Then x=(Ka/c)^0.5

={1.8 x 10^-5/0.1)^0.5 =0.01342

So concetration of H+ ion =Cx

=0.1 x 0.01342 =0.001342

pH=- log(0.001342) =2.87

However it is only an approximate method. Without using approximation, if we solve equation

Ka =Cx^2/1-x , for value of 'x', where C=0.1 then

We get x = 0.01273

So concetration of H+ ion = Cx

=0.1 x 0.01273 =0.001273

pH = - log (0.001273)

= 2.89.

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There will be needed 982.35 mL of solution to obtain 16.1 grams of the salt.There will be needed mL of

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In order to calculate how many milliliters are needed to obtain 16.1 grams of the salt given its concentration, we first need to find its chemical formula which is the following:

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$MolecularMass=\frac{28g+8g+12.01g+47.97g}{mol}=95.98\frac{g}{mol}$

Therefore, knowing the molecular mass of the substance, we need to calculate how many mols represents 16.1 grams of the same substance, we can do it by the following way:

$mol_{(NH_{4})2CO_{3}=\frac{mass_{(NH_{4})2CO_{3}}}{molarmass_{(NH_{4})2CO_{3}}}$

$mol_{(NH_{4})2CO_{3}=\frac{16.1g}{95.98\frac{g}{mol}}=0.167mol$

Finally, if we need to calculate how many milliliters are needed, we need to use the following formula:

$M=\frac{moles_{solute}}{volume_{solution}}$

$M=\frac{moles_{solute}}{volume_{solution}}\\\\volume_{solution}=\frac{moles_{solute}}{M}$

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Calculate the pH of a solution on mixing 0.1 M (50 mL) Ch3cooh and 0.1M(50 mL) NaohKa= 0.00005​

Calculate the pH of a solution on mixing 0.1 M (50 mL) Ch3cooh and 0.1M(50 mL) NaohKa= 0.00005