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Julli [10]
3 years ago
5

Determine whether a precipitate will form when 0.96g of Na2CO3 is combined with 0.20g BaBr2 in a 10 L solution.

Chemistry
1 answer:
Mashcka [7]3 years ago
3 0

Answer:

Qsp > Ksp, BaCO3 will precipitate

Explanation:

The equation of the reaction is;

Na2CO3 + BaBr2 -------> 2NaBr + BaCO3

Since BaCO3 may form a precipitate we can determine the Qsp of the system.

Number of moles of Na2CO3 = 0.96g/106 g/mol = 9.1 * 10^-3 moles

concentration of NaCO3 = number of moles/volume of solution = 9.1 * 10^-3 moles/10 L = 9.1 * 10^-4 M

Number of moles of BaBr2 = 0.20g/297 g/mol = 6.7 * 10^-4 moles

concentration of BaBr2 = 6.7 * 10^-4 moles/10 L = 6.7 * 10^-5 M

Hence;

[Ba^2+] = 6.7 * 10^-5 M

[CO3^2-] = 9.1 * 10^-4 M

Qsp = [6.7 * 10^-5] [9.1 * 10^-4]

Qsp = 6.1 * 10^-8

But, Ksp for BaCO3 is 5.1*10^-9.

Since Qsp > Ksp, BaCO3 will precipitate

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Answer:

0.12M

Explanation:

A balanced equation for the reaction will go a great deal in obtaining our desired result. So, let us write a balanced equation for the reaction

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From the above equation,

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Data obtained from the question include:

Vb (volume of the base) = 30mL

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The molarity of the acid can be obtained as follow:

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Cross multiply to express in linear form

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5 0
3 years ago
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6 0
3 years ago
The mass of an object is 1,000 g. It has a volume of 100 mL. What is the density of the object? D= mass/volume
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Answer:

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