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faust18 [17]
3 years ago
13

The maximum allowable concentration of Pb2+ ions in drinking water is 0.05 ppm (i.e., 0.05 g of Pb2+ in 1 million grams of water

). (a) What is the Pb2+ concentration of an underground water supply at equilibrium with the mineral cerussite (PbCO3) (Ksp = 3.3 × 10−14) ? × 10 g / LEnter your answer in scientific notation. (b) Does this concentration exceed the allowable concentration guideline? Yes No
Chemistry
1 answer:
Diano4ka-milaya [45]3 years ago
6 0

Answer:

a. 0,049g of Pb²⁺ in 1 million grams of water.

b. No

Explanation:

The equilibrium of PbCO₃ in water is:

PbCO₃ ⇄ Pb²⁺ + CO₃²⁻

Where ksp is defined as:

ksp = [Pb²⁺] [CO₃²⁻] <em>(1)</em>

The initial concentration of PbCO₃ in molarity is:

\frac{10g}{1L}×\frac{1mol}{267,21g}= 0,0374M

a. The concentrations in equilibrium are:

[PbCO₃} = 0,0374M-x

[Pb²⁺] = x

[CO₃²⁻] = x

Replacing in (1)

3,3x10⁻¹⁴ = x²

x = 1,82x10⁻⁷M

Thus, [Pb²⁺] = 1,82x10⁻⁷M, this value in g of Pb²⁺ per million grams of water is:

1,82x10⁻⁷M×\frac{267,21g}{1mol}×\frac{1x10^6g}{1000g} = <em>0,049 g of Pb²⁺ in 1 million grams of water</em>

As this value is lower than the maximum allowable concentration of Pb²⁺, <em>the concentration doesn't exceed this maximum value</em>

<em />

I hope it helps!

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Five ?L of a 10-to-1 dilution of a sample were added to 5mL of Bradford reagent. The absorbance at 595 nm was 0.78 and,according
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Answer:

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Five μL of a 10-to-1 dilution of a sample; This implies the Volume of dilute sample is given as 5 μL

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2 years ago
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