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UkoKoshka [18]
3 years ago
13

Find the mass of sucrose (molecular mass=342) required to be dissolved per 600cm² solution to prepare a semi molar solution.

Chemistry
1 answer:
Natalka [10]3 years ago
4 0

Answer:

102.6 g

Explanation:

Firstly, let's understand the terms used in the question. Semi-molar solution is a solution which has a molarity of:

c=\frac{1}{2} M=0.5 M

We're given the molar mass of:

M=342 \frac{g}{mol}

Let's use the definition of molarity: molarity is the ratio between the moles of solute and the volume of solution:

c=\frac{n}{V}

From here, we wish to express moles, n, as the ratio of mass of sucrose to its molar mass:

n=\frac{m}{M}

Substitute it back into the equation of molarity:

c=\frac{n}{V}=\frac{\frac{m}{M} }{V}=\frac{m}{MV}

Since we wish to find mass, let's multiply both sides of the equation by MV to obtain mass equation:

m=cMV

Now, convert volume into liters knowing that 1 mL = 1 cm³ and 1000 mL = 1 L:

600 cm^3 \cdot\frac{1 mL}{1 cm^3} \cdot \frac{1 L}{1000 mL} =0.600 L

Substitute all three variables into the equation:

m=0.5 M\cdot342 \frac{g}{mol}\cdot0.600 L=102.6 g

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Complete question is;

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D) a car with a mass of 5,000 kg

Explanation:

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3 years ago
A 3.4 g sample of an unknown monoprotic organic acid composed of C,H, and O is burned in air to produce 8.58 grams of carbon dio
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Answer:

C_7H_6O_2

Explanation:

Hello there!

In this case, we can divide the problem in three stages: (1) determine the empirical formula with the combustion analysis, (2) compute the molar mass of acid via the moles of the acid in the neutralization and (3) determine the molecular formula.

(1) In this case, since 8.58 g of carbon dioxide are released, we can first compute the moles of carbon in the compound:

n_C=8.58gCO_2*\frac{1molCO_2}{44.01gCO_2}*\frac{1molC}{1molCO_2}=0.195molC

And the moles of hydrogen due to the produced 1.50 grams of water:

n_H=1.50gH_2O*\frac{1molH_2O}{18.02gH_2O}*\frac{2molH}{1molH_2O}  =0.166molH

Next, to compute the mass and moles of oxygen, we need to use the initial 3.4 g of the acid:

m_O=3.4g-0.195molC*\frac{12.01gC}{1molC}-0.166molH*\frac{1.01gH}{1molH} =0.89gO\\\\n_O=0.89gO*\frac{1molO}{16.0gO}=0.0556molO

Thus, the subscripts in the empirical formula are:

C=\frac{0.195}{0.0556}=3.5 \\\\H=\frac{0.166}{0.0556}=3\\\\O=\frac{0.0556}{0.0556}=1\\\\C_7H_6O_2

As they cannot be fractions.

(2) In this case, since the acid is monoprotic, we can compute the moles by multiplying the concentration and volume of KOH:

n_{KOH}=0.279L*0.1mol/L\\\\n_{KOH}=0.0279mol

Which are equal to the moles of the acid:

n_{acid}=0.0279mol

And the molar mass:

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(3) Finally, since the molar mass of the empirical formula is:

7*12.01 + 6*1.01 + 2*16.00 = 122.13 g/mol

Thus, since the ratio of molar masses is 122.86/122.13 = 1, we infer that the empirical formula equals the molecular one:

C_7H_6O_2

Best regards!

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