Acid-Base Reactions

Neutralization is a reaction between an acid and a base. Which equations represent a neutralization reaction? Select all that apply.

• Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)

• H2SO4(aq) + 2KOH(aq) → K2SO4(aq) + 2H2O(l)

• AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)

• 3HCl(aq) + Fe(OH)3(s) → FeCl3(aq) + 3H2O(l)

• HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

Predict the products for the neutralization reactions by filling in the blanks. A. 2HNO3(aq) + Ba(OH)2(aq) → _____ + 2H2O(l)

• Ba(NO3)2(aq)

• Ba(NO2)2(aq)

• BaO(aq)

• Ba(OH)2(aq)

Tags

NGSS.HS-PS1-1

Predict the products for the neutralization reactions by filling in the blanks. B. 2H3PO4(aq) + 3Ca(OH)2(aq) → _____ + 6H2O(l)

• Ca3(PO4)2(aq)

• Ca(PO4)2(aq)

• Ca2(PO4)3(aq)

• Ca3(PO3)2(aq)

Predict the products for the neutralization reactions by filling in the blanks. C. H2SO4(aq) + Sr(OH)2(aq) → _____ + 2H2O(l)

• SrSO4(aq)

• SrSO4(s)

• Sr(OH)2(aq)

• H2SO4(aq)

Tags

NGSS.HS-PS1-1

• increase
• decrease

Tags

NGSS.HS-PS1-5

The equivalence point in a titration of NaOH with a strong acid is found at pH 7. What does the equivalence point represent, and why does the pH increase drastically at this stage?

• It is the point where the acid and base have completely reacted, resulting in a rapid increase in pH due to the addition of excess base.

• It is the point where the solution becomes neutral, and the pH remains constant.

• It is the point where the acid is in excess, causing the pH to decrease.

• It is the point where the base is in excess, causing the pH to decrease.

Tags

NGSS.HS-PS1-5