Pls helpppp!!!!!! :>

Suppose of copper(II) acetate is dissolved in of a aqueous solution of sodium chromate. Calculate the final molarity of acetate

uranmaximum [27]

Answer:

0.0714 M for the given variables

Explanation:

The question is missing some data, but one of the original questions regarding this problem provides the following data:

Mass of copper(II) acetate: $m_{(AcO)_2Cu} = 0.972 g$

Volume of the sodium chromate solution: $V_{Na_2CrO_4} = 150.0 mL$

Molarity of the sodium chromate solution: $c_{Na_2CrO_4} = 0.0400 M$

Now, when copper(II) acetate reacts with sodium chromate, an insoluble copper(II) chromate is formed:

$(CH_3COO)_2Cu (aq) + Na_2CrO_4 (aq)\rightarrow 2 CH_3COONa (aq) + CuCrO_4 (s)$

Find moles of each reactant. or copper(II) acetate, divide its mass by the molar mass:

$n_{(AcO)_2Cu} = \frac{0.972 g}{181.63 g/mol} = 0.0053515 mol$

Moles of the sodium chromate solution would be found by multiplying its volume by molarity:

$n_{Na_2CrO_4} = 0.0400 M\cdot 0.1500 L = 0.00600 mol$

Find the limiting reactant. Notice that stoichiometry of this reaction is 1 : 1, so we can compare moles directly. Moles of copper(II) acetate are lower than moles of sodium chromate, so copper(II) acetate is our limiting reactant.

Write the net ionic equation for this reaction:

$Cu^{2+} (aq) + CrO_4^{2-} (aq)\rightarrow CuCrO_4 (s)$

Notice that acetate is the ion spectator. This means it doesn't react, its moles throughout reaction stay the same. We started with:

$n_{(AcO)_2Cu} = 0.0053515 mol$

According to stoichiometry, 1 unit of copper(II) acetate has 2 units of acetate, so moles of acetate are equal to:

$n_{AcO^-} = 2\cdot 0.0053515 mol = 0.010703 mol$

The total volume of this solution doesn't change, so dividing moles of acetate by this volume will yield the molarity of acetate:

$c_{AcO^-} = \frac{0.010703 mol}{0.1500 L} = 0.0714 M$

8 0

4 years ago

How do you work out the moles of something?

Fittoniya [83]

1 mole of a pure substance has a mass equal to its molecular mass expressed in grams.
This is known as the molar mass, M, and has the units g mol-1
So 2 moles of a substance would have a mass = 2 x molar mass
3 moles of a substance would have a mass = 3 x molar mass etc
This leads to the formula: mass = moles x molar mass
If we let:
m = mass of substance in grams,
n = moles of pure substance,
M = molar mass of the pure substance in g mol-1
we can write the equation: m = n x M
This equation can be rearranged to give the following:
n = m ÷ M (moles = mass ÷ molar mass)
M = m ÷ n (molar mass = mass ÷ moles)

7 0

3 years ago

Imagine that you have a 7.00 L gas tank and a 3.00 L gas tank. You need to fill one tank with oxygen and the other with acetylen

AleksAgata [21]

Answer:

The acetylene must be fill at 315 atm.

Explanation:

Given data:

Pressure of oxygen =P₁= 135 atm

Volume of oxygen = V₁=7.00 L

Volume of acetylene = V₂=3.00 L

Pressure of acetylene =P₂= ?

Solution:

According to Boyle's law

P₁V₁ = P₂V₂

P₂ = P₁V₁/V₂

P₂ = 135 atm × 7.0 L / 3.00 L

P₂ = 945 atm. L/ 3.00 L

P₂ = 315 atm

The acetylene must be fill at 315 atm.

3 0

4 years ago

Many radioactive atoms that have large masses undergo radioactive decay by releasing a particle that is identical to a helium-4

alexira [117]

I think its a half life.

3 0

3 years ago

Draw the Lewis structure with the lowest formal charges for ClF2+ . Include nonzero formal charges and lone pair electrons in th

masya89 [10]

Answer:

See explanation

Explanation:

The formal charge is obtained from;

Formal Charge = Valence electrons on atom - [number of bonds - lone pair electrons]

The correct structure of ClF2+ is the structure attached to this answer (image obtained from quora) in which the formal charge on fluorine is zero and the formal charge on chlorine is + 1. This is the correct structure because the chlorine is more electronegative than fluorine as expected.

4 0

3 years ago

Pls helpppp!!!!!! :> ​

Pls helpppp!!!!!! :>