A 50.0 mL sample of 0.350 M N2H4 (Kb = 9.51 x 10-7) is titrated with...
A 50.0 mL sample of 0.350 M N2H4 (Kb = 9.51 x 10-7) is titrated with 0.500 M HBr. Calculate:
a. the pH after adding 10.00 mL of HBr
b. the pH at one-half the equivalence point
c. the pH after adding 20.00 mL of HBr
d. the volume required to reach the equivalence point
e. the pH at the equivalence point
f. the pH after adding 45.00 mL of HBr
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A 50.0 mL sample of 0.350 M N2H4 (Kb = 9.51 x 10-7) is titrated
with...
A 40.0 mL sample of 0.150 M HNO2 (Ka = 4.60 x 10-4) is titrated with...
A 40.0 mL sample of 0.150 M HNO2 (Ka = 4.60 x 10-4) is titrated with 0.200 M KOH. Calculate: a. the pH after adding 10.00 mL of KOH b. the pH at one-half the equivalence point c. the pH after adding 20.00 mL of KOH d. the volume required to reach the equivalence point e. the pH at the equivalence point f. the pH after adding 45.00 mL of KOH
A 50.0 mL sample of 0.150 M sodium hydroxide is titrated with 0.250 M nitric acid....
A 50.0 mL sample of 0.150 M sodium hydroxide is titrated with 0.250 M nitric acid. Calculate: a. the pH after adding 10.00 mL of HNO3 b. the pH after adding 40.00 mL of HNO3 c. the volume required to reach the equivalence point d. the pH at the equivalence point
A 25.0 mL volume of a 0.200 M N2H4 solution (Kb = 1.70 × 10−6) is...
A 25.0 mL volume of a 0.200 M N2H4
solution (Kb = 1.70 ×
10−6) is titrated to the equivalence point
with 0.100 M HCl. What is the pH of this solution at the
equivalence point? The titration is:
N2H4 + HCl
N2H5+ + Cl−
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A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH...
A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 12.0 mL of KOH. Express your answer numerically. A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 13.0 mL of HNO3. Express your answer numerically. A 52.0-mL volume of 0.35 M CH3COOH (Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 33.0 mL...
Consider the titration of a 25.0 −mL sample of 0.180 M CH3NH2 with 0.150 M HBr....
Consider the titration of a 25.0 −mL sample of 0.180 M CH3NH2 with 0.150 M HBr. Determine each of the following: a) the initial pH b) the volume of added acid required to reach the equivalence point c) the pH at 4.0 mL of added acid d) the pH at one-half of the equivalence point e) the pH at the equivalence point f) the pH after adding 4.0 mLof acid beyond the equivalence point
Consider the titration of a 28.0 −mL sample of 0.170 M CH3NH2 with 0.145 M HBr. Determine each of the following. a) the...
Consider the titration of a 28.0 −mL sample of 0.170 M CH3NH2 with 0.145 M HBr. Determine each of the following. a) the initial ph b)the volume of added acid required to reach the equivalence point c)the pH at 4.0 mL of added acid d)the pH at one-half of the equivalence point e)the pH at the equivalence point f)the pH after adding 6.0 mL of acid beyond the equivalence point
a 50.0 mL sample of a 0.100 M solution of NaCN is titrated by 0.100 M...
a 50.0 mL sample of a 0.100 M solution of NaCN is titrated by 0.100 M HCl. kb for CN is 2.0x10-5. A.calculate the pH of the solution prior to the start of the titration. B after the addition of 10.0 mL. C. after the addition of 25.0 mL of 0.100 M HCl. D. at the equivalence point. E. after the addition of 60.0 mL of 0.100 M HCl
You have 40.00 mL of a 0.300 M aqueous solution of the weak base C6H5NH2 (Kb = 4.00 x 10-10). This solution will be titr...
You have 40.00 mL of a 0.300 M aqueous solution of the weak base C6H5NH2 (Kb = 4.00 x 10-10). This solution will be titrated with 0.300 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution...
A student titrated a 100.0 mL sample of 0.100 M acetic acid with 0.050 M NaOH....
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A 25.0 mL volume of a 0.200 M N2H4
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10−6) is titrated to the equivalence point
with 0.100 M HCl. What is the pH of this solution at the
equivalence point? The titration is:
N2H4 + HCl
N2H5+ + Cl−
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