Answers:
- a.) 10.0 mL of 0.0500 M HCl: 5.00 ml
- b.) 25.0 mL of 0.126 M HNO₃: 31.5 ml
- c.) 50.0 mL of 0.215 M H₂SO4: 215. ml
Explanation:
All the reactions are the neutralization of strong acids with the same strong base.
At the neutralization point you have:
- number of equivalents of the base = number of equivalent of the acid
And the number of equivalents (#EQ) may be calculated using the normality (N) concentration and the volume (V)
Then, at the neutralization point:
- # EQ acid = N acid × V acid
- # EQ base = N base × V base
- N acid × V acid = N base × V base
Also, you can use the formula that relates normality with molarity
- N = M × number of hydrogen or hydroxide ions
<u>a.) 10.0 mL of 0.0500 M HCl</u>
- The number of hydrogen ions for HCl is 1 and the number of hydroxide ions for NaOH is 1.
- 10.0 ml × 0.0500 M × 1 = V base × 0.100 M × 1
⇒ V base = 10.0 ml ×0.0500 M / 0.100 M = 5.00 ml
<u>b.) 25.0 mL of 0.126 M HNO₃</u>
- The number of hydrogen ions for HNO₃ is 1 and the number of hydroxide ions for NaOH is 1.
- 25.0 ml × 0.126 M × 1 = V base × 0.100 M × 1
⇒ V base = 25.0 ml ×0.126 M / 0.100 M = 31.5 ml
<u>c.) 50.0 mL of 0.215 M H₂SO4</u>
- The number of hydrogen ions for H₂SO4 is 2 and the number of hydroxide ions for NaOH is 1.
- 50.0 ml × 0.215 M × 2 = V base × 0.100 M × 1
⇒ V base = 50.0 ml ×0.215 M × 2 / 0.100 M = 215. ml
Answer:
Unbalanced
Explanation:
The reactants side says 2Na. This means there should also be 2Na on the product's side. However, there is only 1 Na there. Therefore, the chemical equations are unbalanced.
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Answer:
a. molecules that gain or lose an atom to develop a bonding charge
Explanation:
