Be sure to answer all parts. find the ph of the equivalence point and the volume (ml) of 0.0895 m koh needed to reach the equivalence point in the titration of 23.4 ml of 0.0390 m hno,. volume: ml koh ph =
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Ответ:
pH = 7
Volume of 0.0895 M KOH = 2.15 mL
Explanation:
(Assuming HNO, should be HNO₃)
The balanced chemical equation is:
HNO₃ + KOH ⇒ H₂O + KNO₃
At the equivalence point, the amount of KOH added is equivalent to the amount of HNO₃ present, which is calculated as follows:
(23.4mL)(0.0390mol/L) = 0.9126 mmol HNO₃
Since HNO₃ and KOH react in a 1:1 molar proportion, 0.9126 mmol of KOH is required to reach the equivalence point. Therefore, the volume of KOH solution required is:
(0.1926mmol) ÷ (0.0895mol/L) = 2.15 mL KOH solution
The HNO₃ and KOH react completely and neither is in excess, so only the products of the reaction remain (H₂O and KNO₃). Since KNO₃ can be considered a neutral salt, the pH at the equivalence point is 7.
Ответ:
= 49.674 g NaCl
Explanation:
From the equation;
1 mole of Sodium metal produces 2 moles sodium chloride
This means;
23 g of Na will produce 116.88 g of NaCl
Therefore;
11.5 g will generate;
= (11.5 × 116.88)/23
= 58.44 g of NaCl
But;
Percentage yield = (Actual yield/Theoretical yield)× 100%
85 /100 = Actual yield /58.44 g
Thus;
Actual yield = 0.85 × 58.44
= 49.674 g NaCl