Question

In: Chemistry

a titration was performed on a 25.0 mL sample of H2SO4 using 17.86 mL of 1.00...

a titration was performed on a 25.0 mL sample of H2SO4 using 17.86 mL of 1.00 M NaOH. what was the concentration of the H2SO4 solution

Solutions

Expert Solution


Related Solutions

Consider the titration of 25.0 mL of aqueous sample of methamphetamine (C10H14NH) with 0.0955M HCl. It...
Consider the titration of 25.0 mL of aqueous sample of methamphetamine (C10H14NH) with 0.0955M HCl. It took 21.25 mL of HCl to reach the equivalence point. Methamphetamine Kb = 1.0 x10^-10 a. Write the balanced net ionic equation for the titration reaction (including states) b. calcuate the molar concentration of methamphetamine in the sample c. calculate the initial pH of the methamphetamine sample d. identify the predominant species that affects the pH at the equivalence point and calculate its molarity...
A 1.00 L sample of a gas at 25.0
A 1.00 L sample of a gas at 25.0
25.0 mL of a 1.00 M Fe(No3)2 solution was reacted with 25.0 mL of a 0.700M...
25.0 mL of a 1.00 M Fe(No3)2 solution was reacted with 25.0 mL of a 0.700M solution of K3PO4 to produce the solid Fe3(PO4)2 by the balanced chemical equation 3 Fe(NO3)2(aq)+ 2 K3PO4(aq)--->Fe3(PO4)2(s)+ 6 KNO3(aq) What is the limiting reagent? How many grams of Fe(PO4)2 will be produced?
Consider the titration of a 25.0 −mL sample of 0.110 M HC2H3O2 with 0.125 M NaOH....
Consider the titration of a 25.0 −mL sample of 0.110 M HC2H3O2 with 0.125 M NaOH. Determine each of the following.(please do all) a)the initial pH b)the volume of added base required to reach the equivalence point c)the pH at 6.00 mL of added base d)the pH at one-half of the equivalence point ,andt he pH at the equivalence point
Consider the titration of a 25.0 −mL sample of 0.110 M HC2H3O2 with 0.130 M NaOH....
Consider the titration of a 25.0 −mL sample of 0.110 M HC2H3O2 with 0.130 M NaOH. Ka(H2C2H3O2) = 1.8x10-5 A) Initial PH B)  the volume of added base required to reach the equivalence point C)   the pH at 4.00 mL of added base D)   the pH at one-half of the equivalence point
Consider the titration of a 25.0 ml sample of 0.175 M CH3NH2 with 0.150 HBr. Determine...
Consider the titration of a 25.0 ml sample of 0.175 M CH3NH2 with 0.150 HBr. Determine each quantity. a) The volume of added acid required to reach the equivalence point. b) The ph at one-half the equivalence point. c) The ph at the equivalent point. d) The ph after adding 5.0 ml of acid beyond the equivalent point.
Consider the titration of a 25.0 −mL sample of 0.100 M HC2H3O2 with 0.120 M NaOH....
Consider the titration of a 25.0 −mL sample of 0.100 M HC2H3O2 with 0.120 M NaOH. Determine each of the following. the initial pH Express your answer using two decimal places. pH = 2.87 B) Part B the volume of added base required to reach the equivalence point in mL? Part C the pH at 4.00 mL of added base Express your answer using two decimal places. Part D the pH at one-half of the equivalence point Express your answer...
mL HCl added pH 0.00 11.86 25.0 10.71 50.0 6.09 A titration of 25.0 mL of...
mL HCl added pH 0.00 11.86 25.0 10.71 50.0 6.09 A titration of 25.0 mL of 0.100 M triethylamine ((CH3CH2)3N) was performed with 0.0500 M HCl. Given the following data calculate the pKa for triethylammonium ion.
Consider the titration of a 25.0 mL sample of 0.100 M CH3COOH (Ka= 1.8e-5) with 0.130...
Consider the titration of a 25.0 mL sample of 0.100 M CH3COOH (Ka= 1.8e-5) with 0.130 M NaOH. Determine the pH after adding 4.0 mL of base beyond the equivalence point.
For the titration of 50.00 mL of a 0.1000 M solution of compound H2SO4 with a...
For the titration of 50.00 mL of a 0.1000 M solution of compound H2SO4 with a 0.2000 M solution of compound NaOH in the following table. For each titration, calculate the pH after the addition of 0.00, 20.00, 25.00, 37.50, 50.00, and 60.00 mL of com- pound NaOH. Please explain all the steps.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT