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
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.
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
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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To determine the identity of the unknown base, we can use the concept of stoichiometry, which involves the balanced chemical equation for the neutralization reaction.
First, let's write the balanced equation for the reaction between the base and nitric acid (HNO3):
Base + HNO3 -> Salt + Water
Since we are given the volume and concentration of the acid (HNO3), we can calculate the amount of acid used (moles) by using the formula:
moles of acid = volume of acid (L) × concentration of acid (M)
In this case, the volume of the acid is 12 mL, which we need to convert to L:
12 mL = 12/1000 L = 0.012 L
Now, let's calculate the moles of HNO3 used:
moles of acid = 0.012 L × 0.150 M = 0.0018 moles
Since the stoichiometry of the balanced equation is 1:1 between the acid and the base, the number of moles of the base is also 0.0018 moles.
Now, let's calculate the concentration of the unknown base:
concentration of base = moles of base / volume of base (L)
Given that the volume of the base is 30 mL, we convert it to L:
30 mL = 30/1000 L = 0.030 L
Now, calculate the concentration of the unknown base:
concentration of base = 0.0018 moles / 0.030 L = 0.060 M
Since the concentration of the unknown base is 0.0300 M and we calculated it to be 0.0600 M, there might be an error in the given concentration. However, assuming the concentration given is correct, the possible identities for the unknown base could be any strong base with a concentration of 0.060 M, such as sodium hydroxide (NaOH), potassium hydroxide (KOH), or calcium hydroxide (Ca(OH)2), among others.