30 ml of sample of unknown strong base is neutralized after the addition of 12 ml of a 0.150 M HNO3 solution if the unknown base concentration 0.0300 M give the possible identities for the unknown base

Answer 1

First, figure out how many moles of acid you used:
0.012 L X 0.150 M = 1.8 X 10^-3 moles.

Now, your base contained 0.030L X 0.0300 M = 9 X 10^-4 moles of base. If your base was NaOH or LiOH, the solution would have contained only 9 X 10^-4 moles of OH- and would have used only 9 X 10^-4 moles of HNO3. So, your strong base had to have 2 OH ions since you needed twice as many moles of HNO3 as you had of base. So, it could be either Ca(OH)2, Sr(OH)2, or Ba(OH)2. It could not have been any of the others.

Answer 2

the concentration of a certain sodium hydroxide solution was determined by using using the solution to titrate a sample of KHP is an acid with one acidic hydrogen and a molar mass of 204.22 g/mol. in the titration 34.67ml of the sodium hydroxide solution required to react with 0.1082 g KHP calculate the molarity of the sodium hydroxide

Answer 3

KHP + NaOH ==> NaKP + H2O
mols KHP = grams/molar mass
mols NaOH = mols KHP since 1 mol KHP = 1 mol NaOH.
M NaOH = mols NaOH/L NaOH
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Answer 4

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