Similar questions Q. What volume of 0.10 MH2SO4 must be added to 50 ml of a 0.10 M NaOH solution to make a solution in which the molarity of theH2SO4 is 0.050 M? Q. What volume of 0.10 M H2SO4 must be added to 50ml of 0.10 M NAOH solution to make a solution in which the molarity H2SO4 is 0.050 M!?
Q. What approximate volume of 0.40 M
Ba(OH)2 must be added to 50.0 mL of 0.30 M NaOH to get a solution in which the molarity of the OH ions is 0.50 M? Q. A
15 mL sample of 0.20M
MgCl2 is added to
45 mL of 0.40M
AlCl3, what is the molarity of
Cl−ions in the final solution? Q. What volume of 0.01 M H2SO4 must be added to 50ml of 0.01M NaOH solution to make a solution in which the molarity of the H2SO4 is 0.050M? Express your answer using two decimal places.  Barium hydroxide is a strong base for both stages of dissociation: #"Ba"("OH")_2(s) -> "Ba"^{2+}+2"OH"^-# So the solution will have 0.20 M hydroxide ions. Now use the autodissociation product for water: #["H"^+]["OH"^-]=1.0xx10^{-14}"M"^# And then #"pH"=-log_{10}(["H"^+]=5.0xx10^{-14})=13.30#. |
What approximate value of 0.40 m ba(oh)2
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