Is the answer 1 or 2? And why.

If 500.0 ml of 0.10 m ca2+ is mixed with 500.0 ml of 0.10 m so42−, what mass of calcium sulfate will precipitate? ksp for caso4

attashe74 [19]

Answer : The mass of calcium sulfate precipitate will be, 6.12 grams

Solution :

First we have to calculate the moles of $Ca^{2+}$ and $SO_4^{2-}$ .

$\text{Moles of }Ca^{2+}=\text{Molarity of }Ca^{2+}\times \text{Volume of }Ca^{2+}=0.10mole/L\times 0.5L=0.05\text{ moles}$

$\text{Moles of }SO_4^{2-}=\text{Molarity of }SO_4^{2-}\times \text{Volume of }SO_4^{2-}=0.10mole/L\times 0.5L=0.05\text{ moles}$

As, 0.05 moles of $Ca^{2+}$ is mixed with 0.05 moles of $SO_4^{2-}$ , it gives 0.05 moles of calcium sulfate.

Now we have to calculate the solubility of calcium sulfate.

The balanced equilibrium reaction will be,

$CaSO_4\rightleftharpoons Ca^{2+}+SO_4^{2-}$

The expression for solubility constant for this reaction will be,

$K_{sp}=(s)\times (s)$

$K_{sp}=(s)^2$

Now put the value of $K_{sp}$ in this expression, we get the solubility of calcium sulfate.

$2.40\times 10^{-5}=(s)^2$

$s=4.89\times 10^{-3}M$

Now we have to calculate the moles of dissolved calcium sulfate in one liter solution.

$\text{Moles of }CaSO_4=\text{Molarity of }CaSO_4\times \text{Volume of }CaSO_4=4.89\times 10^{-3}mole/L\times 1L=4.89\times 10^{-3}\text{ moles}$

Now we have to calculate the moles of calcium sulfate that precipitated.

$\text{Moles of }CaSO_4\text{ precipitated}=\text{Moles of }CaSO_4\text{ present}-\text{Moles of }CaSO_4\text{ dissolved}$

$\text{Moles of }CaSO_4\text{ precipitated}=0.05-4.89\times 10^{-3}=0.045\text{ moles}$

Now we have to calculate the mass of calcium sulfate that precipitated.

$\text{Mass of }CaSO_4\text{ precipitated}=\text{Moles of }CaSO_4\text{ precipitated}\times \text{Molar mass of }CaSO_4$

$\text{Mass of }CaSO_4\text{ precipitated}=0.045moles\times 136g/mole=6.12g$

Therefore, the mass of calcium sulfate precipitate will be, 6.12 grams

5 0

3 years ago

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point)A chemist has 4.43 g of lithium carbonate and must make a 0.0600 mol/L solution.What volume of solution can be made?a) 0.0

ANTONII [103]

Explanation:

A chemist has 4.43 g of lithium carbonate and must prepare a 0.0600 mol/L (or 0.0600 M) solution. We have to find the volume of solution that can be made.

The molarity of a solution is defined like:

molarity = moles of solute/volume of solution in L

We already know the concentration of the solution (it is 0.0600 mol/L) and the volume is our unknown.

volume of solution in L = ?

molarity = 0.0600 mol/L

We still have to convert the mass of lithium carbonate into moles. To do that we will use the molar mass of the compound.

lithium carbonate = Li₂CO₃

mass of Li₂CO₃ = 4.43 g

molar mass of Li₂CO₃ = 73.89 g/mol

moles of Li₂CO₃ = 4.43 g * 1 mol/(73.89 g)

moles of Li₂CO₃ = 0.0600 moles

Finally we can replace the values in the formula and solve it for the volume of solution.

molarity = moles of solute/volume of solution in L

volume of solution in L = moles of solute/molarity

volume of solution in L = 0.0600 mol/(0.0600 mol/L)

volume of solution in L = 1.00 L

Answer: b) 1.00 L

3 0

1 year ago

Use your understanding of the ideal gas law to identify the correct relationships among the variables. Pressure is . Temperature

MAXImum [283]

Answer:

Pressure is inversely proportional to the volume of a gas at constant temperature and number of moles

Temperature is directly proportional to volume at constant pressure and number of moles

Volume is directly proportional to the number of moles of a gas at constant temperature and pressure

Explanation:

The ideal gas law is derived from a combination of the Boyle's, Charles' and Avogadro's law of gases.

Boyle's law states that at constant temperature, the volume of a given mass of gas (number of moles of gas is constant) is inversely proportional to the pressure exerted by the gas.

V ∝ 1/P (at constant n, T)

Charles'law states that at constant pressure, the volume of a given mass of gas (constant amount, n) is directly proportional to the temperature of the gas; V ∝ T (at constant n, P)

Avogadro’s law states that at constant temperature and pressure, the volume of a given mass of gas is directly proportional to the number of moles of gas present; V ∝ n(at constant T, P)

Combining the three equations gives the following relationship: V ∝ nT/P

By inserting a proportionality constant called the molar gas constant, R, in the relationship above, the ideal gas equation is derived as follows:

V = nRT/P or PV = nRT

5 0

3 years ago

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We know that one mole of Oxygen gas contains two moles of O atoms (remember that O is a diatomic element in nature and is writte

tatiyna

Answer:

12.4 × 10∧3 atoms

Explanation:

Given data:

moles of oxygen molecule= 1.0000 x 10-20 mol

atoms =?

Solution:

32 g O2 = 1 mol = 6.02 × 10∧23

1.0000 x 10∧-20 mol × 6.02 × 10∧23 × 2 = 12.4 × 10∧3 atoms

6 0

4 years ago

Which of the following is a product of photosynthesis reaction

SpyIntel [72]

Glucose and Oxygen
Hope this helped you out

5 0

3 years ago

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