希望可以帮下我Exercise 5.What volume of a 0.234M solution of Ba(OH)2 would be required toprecisely neutralize 750.0mL of a 0.7532M solution of the weak acidCH3COO-H?Exercise 6.A 10.00mL sample of stock phosphoric acid solution H3PO4 (aq) isdil

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希望可以帮下我Exercise 5.What volume of a 0.234M solution of Ba(OH)2 would be required toprecisely neutralize 750.0mL of a 0.7532M solution of the weak acidCH3COO-H?Exercise 6.A 10.00mL sample of stock phosphoric acid solution H3PO4 (aq) isdil

希望可以帮下我Exercise 5.What volume of a 0.234M solution of Ba(OH)2 would be required toprecisely neutralize 750.0mL of a 0.7532M solution of the weak acidCH3COO-H?Exercise 6.A 10.00mL sample of stock phosphoric acid solution H3PO4 (aq) isdil
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Exercise 5.What volume of a 0.234M solution of Ba(OH)2 would be required to
precisely neutralize 750.0mL of a 0.7532M solution of the weak acid
CH3COO-H?
Exercise 6.A 10.00mL sample of stock phosphoric acid solution H3PO4 (aq) is
diluted to 50.00mL,and then titrated with a known KOH solution.If 55.58mL
of that 1.554M KOH(aq) solution is required to neutralize all of the acid,what
was the molarity of the original H3PO4 (aq) solution?

希望可以帮下我Exercise 5.What volume of a 0.234M solution of Ba(OH)2 would be required toprecisely neutralize 750.0mL of a 0.7532M solution of the weak acidCH3COO-H?Exercise 6.A 10.00mL sample of stock phosphoric acid solution H3PO4 (aq) isdil
Answer 5.1207.06mL
Process:750.0mL*0.7532M/(0.234M*2)=1207.06mL
Answer 6.2.88M
Process:1.554M*55.58mL/(3*10.00mL)=2.88M

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