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Vadim26 [7]
3 years ago
13

He concentration of pb2+ in a commercially available standard solution is 1.00 mg/ml. what volume of this solution should be dil

uted to 5.0×102 ml to produce a solution in which the concentration of pb2+ is 0.055 mg/l?
Chemistry
1 answer:
Nina [5.8K]3 years ago
6 0

This can be directly solved using the formula:

C1 V1 = C2 V2

where C is concentration and V is volume

 

1.00 mg/ml * V1 = 0.055 mg/1000 ml * (5.0 x 10^2 ml)

V1 = 0.0275 ml

 

<span>So 0.0275 ml is needed to be diluted to 5.0 x 10^2 ml</span>

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Determine the equilibrium constant, Kp, for the following reaction, by using the two reference equations below: 2 NO(g) + O2(g)
klio [65]

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Kp=3.07x10^6

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Hello,

In this case, by knowing the given reference reactions, one could rearrange them as follows:

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N_2(g) + 2O_2(g) \leftrightarrow 2NO_2(g);Kp_3=(8.4x10^{-7})^2=7.056x10^{-13}

Subsequently, to obtain the main reaction, we add the aforementioned reference rearranged reactions as shown below (just as reference):

2NO(g)+N_2(g)+2O_2\leftrightarrow 2NO_2(g)+N_2+O_2

Consequently, the equilibrium constant is computed as:

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8 0
3 years ago
What is the new concentration of a solution of CaSO3 if 10.0 mL of a 2.0 M CaSO3 solution is diluted to 100 ml?
kifflom [539]

Answer: The new concentration of a solution of CaSO_{3} is 0.2 M 10.0 mL of a 2.0 M CaSO_{3} solution is diluted to 100 mL.

Explanation:

Given: V_{1} = 10.0 mL,      M_{1} = 2.0 M

V_{2} = 100 mL,           M_{2} = ?

Formula used to calculate the new concentration is as follows.

M_{1}V_{1} = M_{2}V_{2}

Substitute the values into above formula as follows.

M_{1}V_{1} = M_{2}V_{2}\\10.0 mL \times 2.0 M = M_{2} \times 100 mL\\M_{2} = 0.2 M

Thus, we can conclude that the new concentration of a solution of CaSO_{3} is 0.2 M 10.0 mL of a 2.0 M CaSO_{3} solution is diluted to 100 mL.

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2 years ago
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