1.) What volume (in mL) of a solution 0.143 M in Ca(OH)2 must we use to neutralize 25.2 mL of a solution 0.388 M in H3PO4. 2.) We have 2.34 L of an aqueous NaBr solution. We add an excess of AgNO3. We form 7.44 g of AgBr(s). What was the initial concentration of Br- (in mol/L) in this aqueous NaBr solution? 3.) What is the pH of a 0.110 M solution of the acid HA if its ionization constant, KA, is 0.24 .
1.) What volume (in mL) of a solution 0.143 M in Ca(OH)2 must we use to neutralize 25.2 mL of a solution 0.388 M in H3PO4. 2.) We have 2.34 L of an aqueous NaBr solution. We add an excess of AgNO3. We form 7.44 g of AgBr(s). What was the initial concentration of Br- (in mol/L) in this aqueous NaBr solution? 3.) What is the pH of a 0.110 M solution of the acid HA if its ionization constant, KA, is 0.24 .
Introductory Chemistry: A Foundation
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ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter15: Solutions
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1.) What volume (in mL) of a solution 0.143 M in Ca(OH)2 must we use to neutralize 25.2 mL of a solution 0.388 M in H3PO4.
2.) We have 2.34 L of an aqueous NaBr solution. We add an excess of AgNO3. We form 7.44 g of AgBr(s). What was the initial concentration of Br- (in mol/L) in this aqueous NaBr solution?
3.) What is the pH of a 0.110 M solution of the acid HA if its ionization constant, KA, is 0.24 .
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