1. Calculate the volume in milliliters (mL) of a 6.00 M
NaOH solution needed to make 5.00 x 102 mL of a 0.100 M NaOH
solution. (Recall that M = molar = mol/L, and show all
your work).
2. An approximately 0.1 M NaOH solution was standardized
with KHP by titration to a phenolphthalein endpoint. From the
following data, calculate the average molarity of the NaOH. The
molar mass of KHP is 204.22 g/mol.
Trial 1 Trial 2 Mass of...
A) What volume of 0.456 M HNO3 is needed to titrate 75.00 mL of
1.0x10-3 M Ca(OH)2 to the equivalence point? B) What is the pH of a
buffer system made by dissolving 10.70 grams of NH4Cl and 2.0 mL of
12.0 M NH3 in enough water to make 1.00 L of solution? (Kb=1.8x10-5
for NH3)
500.0 mL of 0.140 M NaOH is added to 565 mL of 0.250 M weak acid
(Ka = 8.39 × 10-5). What is the pH of the resulting buffer?
HA(aq)+OH^-(aq)=H2O(l)+ A^-(aq)
pH=?
20.00 mL of 0.11 M HNO3 is titrated with 0.25 M NaOH. What
volume of base is required to reach the equivalence point?
Calculate pH at each of the following points in the titration.
a) 4.40 mL
b) 8.80 mL
c) 12.00 mL
What volume (in mL) of a 0.125 M HNO3 solution is required to
completely react with 39.8 mL of a 0.102 M Na2CO3 solution
according to the following balanced chemical equation?
Na2CO3(aq)+2HNO3(aq)→2NaNO3(aq)+CO2(g)+H2O(l)
Express your answer with the appropriate units.
A solution is made by mixing 25.0 mL of 0.250 M nitric acid
(HNO3) with 15.0 mL of 0.500 M sodium hydroxide (NaOH). What is the
resulting concentration of each ion in solution?
a) How many moles of water are formed when 28.0 mL of 0.250 M
HNO3 and 53.0 mL of 0.320 M KOH are mixed?
b) What is the concentration of H+(aq) and OH–(aq) after the
reaction is complete?
In a titration 34.20 mL HI, 21.78 mL of 0.250 M LiOH was needed
to reach the equivalence point.
a.) What is the reaction equation for this reaction?
b.) How many moles of LiOH were added during the titration?
c.) How many moles of HI were present in the original
sample?
d.) What was the HI concentration in the original sample?
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