calculate the number of grams of NaOH per 100ml to give a pH8.0 solution if pure

Question

calculate the number of grams of NaOH per 100ml to give a pH8.0 solution if pure water at pH7.0 is used in the experiment. Repeat this calculation for a pH6.0 solution using HCl.

Comment on how this or would not explain the fact that distilled and tap water are not exactly at a pH value of 7.000

Do the Ph values for more dilute solutions approach the ph of distilled water? what would you expect to happen if you continued to dilute these samples even further? explain your answer.

what would you predict if you compared the ph values in a dilution experiment for a strong acid such as HCl and a weak acid such as acetic acid. do the ph values increase at the same rate?

what would you expect to happen if you combined 10.0 ml of 10^-2 M acetic acid and 5.0 ml of 10^-2 M sodium hydroxide? what would be the concentration of acetic acid and sodium acetate in this solution? would you expect this solution to be a buffer? EXPLAIN YOUR PREDICTION.

Explanation / Answer

[OH-]=10^-6

let the concentration of NaOH be c.so,

c+10^-7=10^-6

or c=9*10^-7

so mass persent in 1liter of the solution=40*9*10^-7

=3.6*10^-5 g

so concentration in g/100ml = 3.6*10^-6 g/100ml

b)for HCl,

let the concentration of HCl be c.so,

c+10^-7=10^-6

or c=9*10^-7

so mass persent in 1liter of the solution=36.5*9*10^-7

=3.285*10^-5 g

so concentration in g/100ml = 3.285*10^-6 g/100ml

c)tap water contanis very minute amount of acid or base (depends uopn the region from which the water sample is taken) causig the pH of the water not to be 7   

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