Advanced acids and bases

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if 0.000066 moles of a 0.01 I am solution of carbonic acid dissociates, then what is the Ka of carbonic acid?

0.000066 • 0.000066 / 0.01 = 4.4 • 10^-7

OK. Now let's try harder example. Calculate the pH of 0.02 M methanoic acid where Ka = 1.6 x 10^-4 M

2.75

The logarithmic formula is not as complicated as it seems. For example, what is the pH of a solution with a H+ concentration of 1.00 x 10^-4 M?

4

What is the pH of distilled water?

7

Put acids in order left to right

HCN, H2S, HSO4-, HCl

Mix one acid and one base. sulfate salt

Mix NH3 (unmixed pH =10) and H2SO4 (unmixed pH = 2)

what will be the correct formula to calculate the pH of 100 mL of a 0.03 M solution of nitric acid

PH = - log (0.03)

if equal volumes of a strong base and weaker acid I am mixed together, what would you expect the pH of the resulting salt to be?

PH higher than seven, because there will be fewer [H+] than [OH-]

we learned that pH is related to concentration of the hydrogen ions (H+). what will happen if we lower the hydrogen ion concentration?

The PH will be higher

do you have an idea how we could make the lake less acidic?

add a base

what kind of acid could be formed from these building blocks

carbonic acid

what would be the most sensible response?

how strong is the storm

prepare a neutral calcium salt

mix Ca(OH)2 and H2SO4

mix to make ?

mix H2CO3 and Ca(OH)2

Mix solutions to prepare an acidic chloride salt

mix NH3 and HCl

A 0.0 1M solution of carbonic acid dissociates into 0.000066 moles of HCO3- at equilibrium. What is the pH?

pH = - log (0.000066) = 4.18

after testing multiple samples of control rainwater, it looks like it has an average pH of 5.6. This experiment shows rain is naturally

slightly acidic

A salt solution can either be basic, acidic, or neutral. If a strong acid and strong base produce water and a neutral salt, then what does a weak acid and strong base mix to produce?

water + base salt


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