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3 years ago

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What volume of 5.00 × 10-3 m hno3 is needed to titrate 80.00 ml of 5.00 × 10-3 m ca(oh)2 to the equivalence point? what volume o

f 5.00 × 10-3 m hno3 is needed to titrate 80.00 ml of 5.00 × 10-3 m ca(oh)2 to the equivalence point? 80.0 ml 160. ml 10.0 ml 40.0 ml?

1 answer:

Dimas [21]3 years ago

4 0

Answer:

= 160 mL

Explanation:

The equation for the reaction is;

Ca(OH)2 + 2HNO3 -----> Ca(NO3)2 + 2H2O

Moles of Ca(OH)2 = 0.080 L x 5.00^-3 M

= 0.0004 moles

From the reaction; 2 moles of HNO3 reacts with 1 mole of Ca(OH)2

Thus; moles of HNO3 = 0.0004 Moles × 2

= 0.0008 moles

Volume = moles/ molarity

Therefore; volume of HNO3= 0.0008 Moles/ 5 × 10^-3 M

<u>= 0.16 L or 160 mL</u>

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