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vaieri [72.5K]
3 years ago
6

How many liters of solution will contain 1.5 moles of CaCl2 if the solution is 6.0 M CaCl2?

Chemistry
1 answer:
sashaice [31]3 years ago
6 0

Answer:

0.25

Explanation:

volume= number of moles over concentration

hence v=1.5/6

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Be sure to answer all parts. Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after
Fantom [35]

Answer:

(a) pH = 12.73

(b) pH = 10.52

(c) pH = 1.93

Explanation:

The net balanced reaction equation is:

KOH + HBr ⇒ H₂O + KBr

The amount of KOH present is:

n = CV = (0.1000 molL⁻¹)(30.00 mL) = 3.000 mmol

(a) The amount of HBr added in 9.00 mL of 0.1000 M HBr is:

(0.1000 molL⁻¹)(9.00 mL) = 0.900 mmol

This amount of HBr will neutralize an equivalent amount of KOH (0.900 mmol), leaving the following amount of KOH:

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C = n/V = (2.100 mmol) / (39.00 mL) = 0.0538461 M KOH

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pH = 14 - pOH = 14 - 1.2688 = 12.73

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(c) The amount of HBr added in 38.00 mL of 0.1000 M HBr is:

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C = n/V = (0.800 mmol) / (68.00 mL) = 0.01176 M HBr

The pH of the solution can then be calculated:

pH = -log[H⁺] = -log(0.01176) = 1.93

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