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3 years ago

15

In an aqueous solution of a certain acid with pka = 3.75 the ph is 2.82 . calculate the percent of the acid that is dissociated

in this solution. round your answer to significant digits.

1 answer:

Arturiano [62]3 years ago

8 0

Hello! Let me try to answer this :)

Thanks and please correct if there are any mistakes ^ ^

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The molarity of a solution that contains 8.0 g of NaOH in a liter of solution is

Kay [80]

Answer:

0.2M NaOh

Explanation:

there are 0.2 mol of NaOH in 8.0 g. (8.0/40) =0.2. Molarity = mol/L = 0.2M.

8 0

2 years ago

1. identify whether following have ionic or covalent bonding. Give your reasons: Oxygen molecule, water, calcium oxide, hydrogen

Romashka [77]

First you need to know the different between an ionic and covalent bond. An ionic bond is the pairing of a metal and non-metal element. A covalent bond is the pairing of 2 nonmetals.

Metals are the elements at the left of the periodic table while non-metals are the elements at the right of the periodic table.

You should also know the diatomic (di means 2) molecules also known as the fab 7. These molecules will always form covalent bonds. These molecules are hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, and iodine. With the subscripts, these molecules would be written as H ₂, N ₂, O ₂, F ₂, Cl ₂, Br ₂, and I ₂.

5 0

3 years ago

g If 50.0 mL of a 0.75 M acetic acid solution is titrated with 1.0 M sodium hydroxide, what is the pH after 10.0 mL of NaOH have

V125BC [204]

Answer:

pH = 2.66

Explanation:

Acetic Acid + NaOH → Sodium Acetate + H₂O

First we <u>calculate the number of moles of each reactant</u>, using the <em>given volumes and concentrations</em>:

0.75 M Acetic acid * 50.0 mL = 37.5 mmol acetic acid

1.0 M NaOH * 10.0 mL = 10 mmol NaOH

We<u> calculate how many acetic acid moles remain after the reaction</u>:

37.5 mmol - 10 mmol = 27.5 mmol acetic acid

We now <u>calculate the molar concentration of acetic acid after the reaction</u>:

27.5 mmol / (50.0 mL + 10.0 mL) = 0.458 M

Then we <u>calculate [H⁺]</u>, using the<em> following formula for weak acid solutions</em>:

[H⁺] = $\sqrt{C*Ka}=\sqrt{0.458M*1.76x10^{-5}}$

[H⁺] = 0.0028

Finally we <u>calculate the pH</u>:

pH = -log[H⁺]

pH = 2.66

8 0

2 years ago

What is the mass of 4.5 x 10^22 molecules of hydrogen peroxide (H2O2)? Show your work in the space below.

valentinak56 [21]

Given :

Number of molecules of hydrogen peroxide, N = 4.5 × 10²².

To Find :

The mass of given molecules of hydrogen peroxide.

Solution :

We know, 1 mole of every compound contains Nₐ = 6.022 × 10²³ molecules.

So, number of moles of hydrogen peroxide is :

$n = \dfrac{N}{N_a}\\\\n = \dfrac{4.5\times 10^{22}}{6.022\times 10^{23}}\\\\n = 0.0747 \ moles$

Now, mass of hydrogen peroxide is given as :

m = n × M.M

m = 0.0747 × 34 grams

m = 2.54 grams

Hence, this is the required solution.

6 0

3 years ago

Two different compounds are obtained by combining nitrogen with oxygen. the first compound results from combining 46.7 g of n wi

kondaur [170]

<span>First:

46.7 g of N with 53.3 g of O,

=> mass ratio O to N = 53.3 / 46.7 = 1.1413

Second

17.9 g of N and 82.0 g of O.

mass ratio of O to N = 82.0 / 17.9 = 4.5810

Third

Ratio of the mass ratio of O to N in the second compound to the mass ratio of O to N in the first compound =

= 4.5810 / 1.1413 = 4.013 ≈ 4

Answer: 4
</span>

8 0

3 years ago