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shtirl [24]
3 years ago
15

What is the pH of a solution made by diluting 1.00 mL of 0.10 M HCl with enough distilled water to make 1.00 L of solution?

Chemistry
1 answer:
yKpoI14uk [10]3 years ago
3 0

Answer:

The answer to your question is  pH = 4

Explanation:

Data

Volume 1 = V1 = 1 ml = 0.001 l

Concentration 1 = C1 = 0.1 M

Volume 2 = V2 = 1 l

Concentration 2 = C2 = ?

Process

1.- Find the new concentration of the solution

                    C₁V₂  = C₂V₂

Solve for C₂

                     C₂ = C₁V₁ / V₂

Substitution

                     C₂ = (0.1 x 0.001) / 1

Result

                     C₂ = 0.0001 M

2.- Find the pH of the solution

Formula

                pH = -log[H⁺]

Substitution

                pH = - log[0.0001]

Simplification

                pH = 4                  

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natta225 [31]
Answer:  
The balanced equation tells us that 1 mole of Zn will produce 1 mole of H2.  
1.566 g Zn x (1 mole Zn / 65.38 g Zn) = 0.02395 moles Zn  
0.02395 moles Zn x (1 mole H2 / 1 mole Zn) = 0.02395 moles H2 produced  
Now use the ideal gas law to find the volume V.  
P = 733 mmHg x (1 atm / 760 atm) = 0.964 atm  
T = 21 C + 273 = 294 K  
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V = nRT/ P = (0.02395 moles H2)(0.0821 L atm / K mole)(294 K) / (0.964 atm) = 0.600 L
7 0
3 years ago
How many liters of CO2 gas can be produced at 30.0 °C and 1.50 atm from the reaction of 5.00 mol of C3H8 and an excess of O2 acc
lbvjy [14]

Answer:

249 L

Explanation:

Step 1: Write the balanced equation

C₃H₈(g) + 5 O₂(g) → 3 CO₂(g) + 4 H₂O(g)

Step 2: Calculate the moles of CO₂ produced from 5.00 moles of C₃H₈

The molar ratio of C₃H₈ to CO₂ is 1:3. The moles of CO₂ produced are 3/1 × 5.00 mol = 15.0 mol

Step 3: Convert "30.0°C" to Kelvin

We will use the following expression.

K = °C + 273.15

K = 30.0°C + 273.15 = 303.2 K

Step 4: Calculate the volume of carbon dioxide

We will use the ideal gas equation.

P × V = n × R × T

V = n × R × T/P

V = 15.0 mol × 0.0821 atm.L/mol.K × 303.2 K/1.50 atm

V = 249 L

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