3 years ago

Express the following concentration of solution in terms of molarity: 3.00 L of solution contains 1.75 mol of solute.

Chemistry

1 answer:

DENIUS [597]3 years ago

5 0

Great to know when Im in college nobody will answer my tough questions

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Explanation:

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3 years ago

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2. What is the molarity of 100 mL of a 3.0% H2O2 (mass/volume) solution? What is the molarity of 100 mL of a 2.25% H2O2 solution

KatRina [158]

The 3% mass/volume H₂O₂ means 3 g of H₂O₂ in 100 ml of water.

Now, Molarity (M) = No. of moles of H₂O₂ / Volume of solution in liter

No. of moles of H₂O₂ = Mass / Molar mass = 3 g / 34 g/mol = 0.088 mol

So, molarity = 0.088 × 1000 ml / 100 ml = 0.88 M

In case of 2.25 % H₂O₂,

No of moles = 2.25 g / 34 g/mol = 0.066 mol

Molarity = 0.066 mol / 0.100 L = 0.66 M.

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3 years ago

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4 years ago

Find the [H+] in an acetic acid solution that has a pH of 5.12

Eva8 [605]

Data:
pH = 5.2
[H+] = ?

Knowing that: (Equation to find the pH of a solution)
$pH = -log[H+]$

Solving:
 $pH = -log[H+]$
$5.2 = - log [H+]$
Knowing that the exponential is the opposite operation of the logarithm, then we have:
$[H+] = 10^{-5.2}$
$\boxed{\boxed{[H+] = 6.30*10^{-6}}}\end{array}}\qquad\quad\checkmark$

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3 years ago

What is the [H+] concentration of blood, given the ph is 2.5?

belka [17]

Answer:

0.00316

Explanation:

You have to use the following equation:

$pH=-log[H^+]$

You are given the pH and need to find the concentration of H+. Plug in the given components and solve.

$2.5=-log[H^+]\\H^+ = 10^{-2.5}\\H^+=0.00316$

The concentration of H is 0.00316.

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3 years ago