What volume of each of the following acids will react completely with 50.34 mL of 0.111 M NaOH?
a) 0.150 M H2SO3 (two acidic hydrogens)
b) 0.210 M H3PO4 (three acidic hydrogens)
c) 0.315 M H2SO4 (two acidic hydrogens)
What volume of each of the following acids will react completely with 50.34 mL of 0.111...
69. What volume of each of the following acids will react completely with 50.00 mL of 0.200 M NaOH? a. 0.100 M HCI b. 0.150 M HNO3 c. 0.200 M HC2H302 (1 acidic hydrogen)
70. What volume of each of the following bases will react completely with 25.00 mL of 0.200 M HCI? a. 0.100 M NaOH b. 0.0500 M Ba(OH)2 c. 0.250 M KOH
3. Wha t is the reason strong acids react with CaCOs (s) faster than weak acids? a. strong acids are more concentrated b. for solutions of equal concentrations, strong acids have more H3O ions c. strong acids form solids with insoluble ions d. weak acids react with water, and therefore don't react with the CaCOs (s) 4. How much of a 0.100 M NaOH solution is required to completely neutralize 10.0 mL of 0.200 M H2SO4? No calculations are necessary....
1. Determine the volume (mL) of 0.400 M H2SO4 acid required to react completely with 128.0 mL of 0.525 M NaOH base solution. Ans: 82.0 mL H2SO4 (aq) + 2NaOH (aq) → Na2SO4 (aq) + 2H20 (1)
What volume (in mL) of a 0.150 M HNO3 solution will completely react with 36.3 mL of a 0.120 M Na2CO3 solution according to this balanced chemical equation? Na2CO3(aq)+2 HNO3(aq)→2 NaNO3(aq)+CO2(g)+H2O(l)
If a 17.5 mL sample of 1.2 M solution of each of the following acids is reacted with 0.85 M NaOH, how many milliliters of the NaOH are required for the titration? What is the total volume (in mL) of solution at the equivalence point? (a) 17.5 mL of HF titrated with 0.85 M NaOH volume of NaOH mL total volume mL (b) 17.5 mL of H2SO4 titrated with 0.85 M NaOH volume of NaOH mL total volume mL c)...
1. How many milliliters of 0.112 M Na2CO3 will completely react with 27.2 mL of 0.135 M HNO3 according to the reaction 2HNO3(aq) + Na2CO3(aq) → H2O(l) + CO2(g) + 2NaNO3(aq) Part B.) A 25.0-mL sample of HNO3 solution requires 35.7 mL of 0.108 M Na2CO3 to completely react with all of the HNO3 in the solution. What is the concentration of theHNO3 solution? Part C.)Consider the reaction HCl(aq) + NaOH(aq) → NaOH(aq) + H2O(l) How much 0.113 M NaOH...
If a 16.5 mL sample of 1.1 M solution of each of the following acids is reacted with 0.75 M NaOH, how many milliliters of the NaOH are required for the titration? What is the total volume (in mL) of solution at the equivalence point? 16.5 ml H2SO4 titrated with 0.75 M NaOH Volume of NaOH (ml) 24.2 (incorrect) Total Volume (ml) 40.7 (incorrect)
If a 19.5 mL sample of 1.5 M solution of each of the following acids is reacted with 0.80 M NaOH, how many milliliters of the NaOH are required for the titration? What is the total volume (in mL) of solution at the equivalence point? 19.5 mL of H2SO4 titrated with 0.80 M NaOH: volume of NaOH ______ mL total volume______ mL 19.5 mL of HC2H3O2 titrated with 0.80 M NaOH: volume of NaOH_____ mL total volume ____mL 19.5 mL...
If a 16.5 mL sample of 1.3 M solution of each of the following acids is reacted with 0.90 M NaOH, how many milliliters of the NaOH are required for the titration? What is the total volume (in mL) of solution at the equivalence point? 16.5 mL of HCl titrated with 0.90 M NaOH volume of NaOH ___mL total volume___ mL 16.5 mL of H2SO4 titrated with 0.90 M NaOH volume of NaOH ___mL total volume____ mL 16.5 mL of...