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kvv77 [185]
2 years ago
12

A scientist has 500 mL of a 2.1 M stock solution. She dilutes the solution, and the volume of the solution after the dilution is

3.25 L. What is the molarity (M) of the diluted solution?
Chemistry
1 answer:
Liono4ka [1.6K]2 years ago
4 0

The molarity of the diluted solution is 0.32 M

Considering the question given above, the following data were obtained:

Volume of stock solution (V₁) = 500 mL

Molarity of stock solution (M₁) = 2.1 M

Volume of diluted solution (V₂) = 3.25 L = 3.25 × 1000 = 3250 mL

<h3>Molarity of diluted solution (M₂) =....? </h3>

The molarity of the diluted solution can be obtained as follow:

<h3>M₁V₁ = M₂V₂</h3>

2.1 × 500 = M₂ × 3250

1050 = M₂ × 3250

<h3>Divide both side by 3250</h3><h3 />

M₂ = 1050 / 3250

<h3>M₂ = 0.32 M</h3>

Therefore, the molarity of the diluted solution is 0.32 M

Learn more: brainly.com/question/22325751

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Consider the following reaction: NO( g) + SO 3( g) ⇌ NO 2( g) + SO 2( g) A reaction mixture initially contains 0.86 atm NO and 0
DIA [1.3K]

Answer:

The equilibrium pressure of NO2 is 0.084 atm

Explanation:

Step 1: Data given

A reaction mixture initially contains 0.86 atm NO and 0.86 atm SO3.

Kp = 0.0118

Step 2: The balanced equation

NO( g) + SO3( g) ⇌ NO2( g) + SO2( g)

Step 3: The initial pressures

p(NO) = 0.86 atm

p(SO3) = 0.86 atm

p(NO2) = 0 atm

p(SO2) = 0 atm

Step 4: The pressure at the equilibrium

For 1 mol NO we need 1 mol SO3 to produce 1 mol NO2 and 1 mol SO2

p(NO) = 0.86 -x atm

p(SO3) = 0.86 -xatm

p(NO2) = x atm

p(SO2) = x atm

Step 5: Define Kp

Kp = ((pNO2)*(pSO2)) / ((pNO)*(pSO3))

Kp = 0.0118 = x²/(0.86 - x)²

X = 0.08427

p(NO) = 0.86 -0.08427 = 0.77573 atm

p(SO3) = 0.86 -0.08427 = 0.77573 atm

p(NO2) = 0.08427 atm

p(SO2) = 0.08427 atm

The equilibrium pressure of NO2 is 0.08427 atm ≈ 0.084 atm

5 0
3 years ago
Is the water density higher than the aluminum density
posledela
No
Water’s density is 1 g/cm3 and AL is 2700kg/m3
8 0
3 years ago
If you need 0.0592 moles of nitrogen, how many grams of nitrogen do you need to mass(weigh) on the
navik [9.2K]
Urchin tc yc you txutxurzyrxtuciyvuoxutxurx
8 0
2 years ago
Calculate the mass of sodium phosphate in aqueous solution to fully react with 37 g of chromium nitrate(III) an aqueous solution
Alla [95]

Answer:

41 g

Explanation:

The equation of the reaction is;

Cr(NO3)3(aq)+Na3PO4(aq)=3NaNO3(s)+CrPO4(aq)

Number of moles of chromium nitrate = 37g/ 146.97 g/mol = 0.25 moles

1 mole of sodium phosphate reacts with 1 mole of chromium nitrate

x moles of sodium phosphate react as with 0.25 moles of chromium nitrate

x= 1 × 0.25/1

x= 0.25 moles

Mass of sodium phosphate = 0.25 moles × 163.94 g/mol

Mass of sodium phosphate = 41 g

4 0
3 years ago
**PLATO QUESTION, PLEASE ANSWER CORRECTLY, THANK YOU**
marta [7]

<em>PLATO ANSWERS: </em>

<u>A.</u> Which source of electricity generation caused the most emissions?

<u>B.</u> What types of industries are responsible for greenhouse gas emissions?

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<em>Hope I helped some, Have a great day!</em>

7 0
3 years ago
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