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enot [183]
3 years ago
9

How many grams of Ca(NO3)2 are needed to make 25.0 g of a 15.0% Ca(NO3)2(aq)?

Chemistry
1 answer:
yarga [219]3 years ago
5 0

Answer:

3.75 g.

Explanation:

<em>mass percent is the ratio of the mass of the solute to the mass of the solution multiplied by 100.</em>

<em />

<em>mass % = (mass of solute/mass of solution) x 100.</em>

<em></em>

mass of calcium nitrite = ??? g,

mass of the solution = 25.0 g.

∴ mass % = (mass of solute/mass of solution) x 100

<em></em>

<em>∴ mass of solute (calcium nitrite) = (mass %)(mass of solution)/100</em> = (15.0 %)(25.0 g)/100 = <em>3.75 g.</em>

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A 10.0 mL sample of household ammonia solution required38.50 mL of 0.311 M HCl to achieve neutralization. Calculate (a).the mola
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Answer:

a) 1.1974 M

b) 2.07%

Explanation:

In this case, we have a neutralization reaction between the HCl and ammonia, the acid base reaction is as follow:

HCl + NH₃ --------> NH₄⁺ + Cl⁻

a) As we can see, we have a 1:1 mole ration between the acid and the base, therefore we can use the following expression to calculate concentration of the ammonia:

M₁V₁ = M₂V₂

Replacing the data in here, we can solve for the concentration of ammonia:

M₂ = M₁V₁ / V₂

M₂ = 0.311 * 38.50 / 10

M₂ = 1.1974 M

This is the concentration of the ammonia solution.

b) Now we want to know the mass percent, in this case, we need to calculate the moles of ammonia first, and then, turn it into mass using the molar mass given (17 g/mol):

n = 1.1974 * 0.010 = 0.011974 moles

m = 0.011974 * 17 = 0.2036 g

The solution has a density of 0.983 g/mL and we have 10 mL therefore, we should have of mass:

d = m/V

m = d * V

m = 0.983 * 10 = 9.83 g

Finally the mass percent will be:

% = 0.2036 / 9.83 * 100

% = 2.07%

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3 years ago
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Explanation:

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2 years ago
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Answer:

option A = S(s) + O₂(g)   →   SO₂ (s)

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S(s) + O₂(g)   →   SO₂ (s)

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Uses of sulfur dioxde:

It is used as a solvent and reagent in laboratory.

Sulfur dioxide is used to produce sulfuric acid.

It is used as a disinfectant

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7 0
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77.In the early days of automobiles, illumination at night was provided by burning acetylene, C2H2. Though no longer used as aut
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Answer:

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