A. In any solution of HCl in water weâd expect to find not only H+ but also Clâ What concentration of Clâ would you expect to observe in a solution of HCl with an initial concentration of 1.00 x 10â8 M in water?
B. In a solution containing water as the solvent weâd also expect to find some concentration of OHâ. Write a mathematical expression that would permit you to calculate [OHâ] if you knew [H+].
C. If you were to handle a bottle containing an HCl solution in water that was initially 1.00 x 10â8 M it is unlikely that you would get an electrical shock from it, so it must be that the number of positive ions in the bottle exactly equals the number of negative ions. So write a mathematical expression representing this equality that takes into account all the ions present in a 1.00 x 10â8 M solution of HCl in water. You obtained a value for [Clâ] and an expression for [OHâ] above, so plug those in and solve for [H+]. What result does this approach give for the pH of a 1.00 x 10â8 M HCl solution in water? Does this value seem more reasonable than that which you obtained in Key Question 3? If so, in what way is it more reasonable?
1. Use the approach in Key Questions (AâC) to calculate the pH of a solution of HCl in water thatâs initially 1.00 x 10â3 M. Is the result reasonable based on your chemical intuition?
A. In any solution of HCl in water weâd expect to find not only H+ but also Clâ What concentration of Clâ would you expect to observe in a solution of HCl with an initial concentration of 1.00 x 10â8 M in water?
B. In a solution containing water as the solvent weâd also expect to find some concentration of OHâ. Write a mathematical expression that would permit you to calculate [OHâ] if you knew [H+].
C. If you were to handle a bottle containing an HCl solution in water that was initially 1.00 x 10â8 M it is unlikely that you would get an electrical shock from it, so it must be that the number of positive ions in the bottle exactly equals the number of negative ions. So write a mathematical expression representing this equality that takes into account all the ions present in a 1.00 x 10â8 M solution of HCl in water. You obtained a value for [Clâ] and an expression for [OHâ] above, so plug those in and solve for [H+]. What result does this approach give for the pH of a 1.00 x 10â8 M HCl solution in water? Does this value seem more reasonable than that which you obtained in Key Question 3? If so, in what way is it more reasonable?
1. Use the approach in Key Questions (AâC) to calculate the pH of a solution of HCl in water thatâs initially 1.00 x 10â3 M. Is the result reasonable based on your chemical intuition?
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