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3 years ago

The following procedure was carried out to determine thevolume

Chemistry

1 answer:

Goshia [24]3 years ago

8 0

Answer: Volume of the flask is 31.34 mL.

Explanation:

Weight of empty flask $w_1$ = 56.12 grams

Weight of flask with water $w_2$ = 87.39 grams

Weight of water $w_3$ = $w_2-w_1$ = (87.39 - 56.12) grams= 31.27 grams

Density of water = 0.9976 g/mL

0.9976 grams are contained in = 1 ml of water

Thus 31.27 grams are contained in = $\frac{1}{0.9976}\times 31.27=31.34$ ml of water.

Thus the volume of the flask is 31.34 mL.

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ElenaW [278]

Explanation:

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Step 1: Wind moves the blades of the turbine.

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7 0

3 years ago

To measure the amount of calcium carbonate in a seashell, an analytical chemist crushes a sample of the shell to a fine powder a

andreyandreev [35.5K]

The given question is complete, the complete question is:

To measure the amount of calcium carbonate (CaCO) in a seashell, an analytical chemist crushes a 4.80 g sample of the shell to a fine powder and titrates it to the endpoint with 515. mL of 0.140 M hydrogen chloride (HCl) solution. The balanced chemical equation for the reaction is: 2HCI(a)Co (a) H2Co,(aq) + 2Cl (aq)

What kind of reaction is this?

If you said this was a precipitation reaction, enter the chemical formula of the precipitate.

If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base.

If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized

Calculate the mass percent of CaCO in the sample. Be sure your answer has the correct number of significant digits.

Answer:

It is an acid-base reaction and the mass percent of CaCo3 is 75.2%.

Explanation:

A chemical reaction in which an insoluble salt produces from two soluble salts is termed as precipitation reaction.

A reaction in which atleast exchange of one proton takes place between the two species is termed as an acid-base reaction.

A reaction in which any of the element has a change in oxidation state is termed as redox reaction.

In the mentioned reaction, there is a transfer of H⁺, no precipitation is forming, and no change in oxidation state taking place, thus, it is an acid-base reaction.

In the acid-base reaction, the base refers to the species that accepts hydrogen ion or proton. In the given case, CO₃²⁻ is accepting H+ ion to become H₂CO₃. Hence, CO₃²⁻ is the base.

In order to calculate mass percent of CaCO₃, first there is a need to find the moles of HCl reacted for a solution,

Moles = Molarity × Volume (L)

Moles = 0.140 mol/L × 515 × 10⁻³ L

Moles = 0.0721 mol

Now from the balanced equation, one mole of CaCO₃ needs two moles of HCl.

So, moles of CaCO₃ reacted will be,

= 1/2 × 0.0721 = 0.03605 mol

The mass of calcium carbonate taking part in reaction will be,

= Moles × Molar mass

= 0.03605 × 100 gram/mole

= 3.6086 gram

Mass% of CaCO₃ = Mass of CaCO₃/Mass of sample × 100

= 3.6086 grams/4.80 grams × 100

Mass % = 75.2%

3 0

3 years ago

A solution is prepared by dissolving 27.0 g of urea [(NH2)2CO], in 150.0 g of water. Calculate the boiling point of the solution

andrew11 [14]

<u>Answer:</u> The boiling point of solution is 101.56°C

<u>Explanation:</u>

Elevation in boiling point is defined as the difference in the boiling point of solution and boiling point of pure solution.

The equation used to calculate elevation in boiling point follows:

$\Delta T_b=\text{Boiling point of solution}-\text{Boiling point of pure solution}$

To calculate the elevation in boiling point, we use the equation:

$\Delta T_b=iK_bm$

Or,

$\text{Boiling point of solution}-\text{Boiling point of pure solution}=i\times K_b\times \frac{m_{solute}\times 1000}{M_{solute}\times W_{solvent}\text{ (in grams)}}$

where,

Boiling point of pure water = 100°C

i = Vant hoff factor = 1 (For non-electrolytes)

$K_b$ = molal boiling point elevation constant = 0.52°C/m.g

$m_{solute}$ = Given mass of solute (urea) = 27.0 g

$M_{solute}$ = Molar mass of solute (urea) = 60 g/mol

$W_{solvent}$ = Mass of solvent (water) = 150.0 g

Putting values in above equation, we get:

$\text{Boiling point of solution}-100=1\times 0.52^oC/m\times \frac{27\times 1000}{60\times 150}\\\\\text{Boiling point of solution}=101.56^oC$

Hence, the boiling point of solution is 101.56°C

5 0

4 years ago

Compared to the boiling point of 1.0 M KCl(aq) at standard pressure, the boiling point of 1.0 M CaCl2(aq) at standard pressure i

astra-53 [7]

Lower as KCl has ionic bonding which is less stable than CaCl2s covalent bond which requires less energy.

6 0

3 years ago

What is the ph of 0.51 m ca(ch3coo)2 solution?

Sidana [21]

Answer : The pH of calcium acetate solution will be 9.38.

Explanation : When calcium acetate dissocates completely in solution to form Calcium(+2) ions and two acetate ions, this gives the acetate ion concentration as (2 X 0.51 M) = 1.02 M

Acetate ion then hydrolyzes as follows;

$C_{2}H_{3}O_{2}^{-} + HOH HC_{2}H_{2}O_{2} + OH^{-}$ :