Suppose HX is a strong acid. What is the net-ionic equation for the reaction between HX and NaCl? a) H+(aq) + NaCl(aq) ⟶⟶HCl(aq) + Na+(aq) b) HX(aq) + Cl-(aq) ⟶⟶HCl(aq) + X-(aq) c) There is no net ionic equation. d) H+(aq) + Cl-(aq) ⟶⟶HCl(aq)
Suppose HX is a strong acid. What is the net-ionic equation for the reaction between HX and NaCl? a) H+(aq) + NaCl(aq) ⟶⟶HCl(aq) + Na+(aq) b) HX(aq) + Cl-(aq) ⟶⟶HCl(aq) + X-(aq) c) There is no net ionic equation. d) H+(aq) + Cl-(aq) ⟶⟶HCl(aq)
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
Suppose HX is a strong acid. What is the net-ionic equation for the reaction between HX and NaCl?
a) H+(aq) + NaCl(aq) ⟶⟶HCl(aq) + Na+(aq)
b) HX(aq) + Cl-(aq) ⟶⟶HCl(aq) + X-(aq)
c) There is no net ionic equation.
d) H+(aq) + Cl-(aq) ⟶⟶HCl(aq)
Expert Solution
Step 1
Concept: Salts that are from by the reaction of strong bases and strong acids do not hydrolyze.
The pH will remain neutral at 7. Halides and alkaline metals dissociate.But do not affect the H+ as the cation does not alter the H+ and the anion does not attract the H+ from water.
This is why NaCl is a example of neutral salt.
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