Advanced acids and bases
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
