What is the complete ionic equation for the reaction of hydrochloric acid with potassium hydroxide?

Answer 1

# H^+ + Cl^- + K^+ + OH^- = K^+ Cl^- + H_2O#

Hydrochloric acid is HCl. This is an ionic substance so in water it breaks apart into ions # H^+ + Cl_- #
Potassium Hydroxide is also an ionic substance it also breaks apart in water into ions #K^+ + OH^- #

Thus, the reaction's entire ionic equation is

# H^+ + Cl^- + K^+ + OH^- = K^+ + Cl^- + H_2O#

Water is created when hydrogen and oxide ions combine.

The equation for net ions is

#H^+ + OH^- = H_2O#
This is because the # Cl^- + K^+# ions do not undergo any changes therefore are not part of the net ionic equation.
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Answer 2

The entire ionic equation for the reaction between potassium hydroxide (KOH) and hydrochloric acid (HCl) is as follows: H⁺(aq) + Cl⁻(aq) + K⁺(aq) + OH⁻(aq) → H₂O(l) + K⁺(aq) + Cl⁻(aq)

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Answer 3

The complete ionic equation for the reaction of hydrochloric acid with potassium hydroxide is:

( H^+(aq) + Cl^-(aq) + K^+(aq) + OH^-(aq) \rightarrow H_2O(l) + K^+(aq) + Cl^-(aq) )

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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