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3 years ago

3. Suppose you had titrated your vinegar sample with barium hydroxide instead of sodium hydroxide:

Chemistry

1 answer:

charle [14.2K]3 years ago

6 0

Answer:

39.6 mL

Explanation:

Step 1: Write the balanced neutralization reaction

Ba(OH)₂(aq) + 2 CH₃COOH(aq) ⟶ Ba(CH₃COO)₂(aq) + 2 H₂O(l)

Step 2: Calculate the moles corresponding to 2.78 g of CH₃COOH

The molar mass of CH₃COOH is 60.05 g/mol.

2.78 g × 1 mol/60.05 g = 0.0463 mol

Step 3: Calculate the moles of Ba(OH)₂ needed to react with 0.0463 moles of CH₃COOH

The molar ratio of Ba(OH)₂ to CH₃COOH is 1:2. The moles of Ba(OH)₂ needed are 1/2 × 0.0463 mol = 0.0232 mol.

Step 4: Calculate the volume of 0.586 M solution that contains 0.0232 moles of Ba(OH)₂

0.0232 mol × 1 L/0.586 mol = 0.0396 L = 39.6 mL

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Calculate the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO3) and 0.278 M in potassium n

RideAnS [48]

Explanation:

Concentration of $KNO_{2}$ is 0.278 M and it is completely ionized into $K^{+}$ and $NO^{-}_{2}$ .

This means that $[KNO_{2}]$ = $[NO_{2}]$ = 0.278 M

It is given that concentration of $HNO_{2}$ is 0.222 M.

As $HNO_{2}$ is a weak acid. Therefore, its dissociation will be as follows.

$HNO_{2}(aq) \rightarrow H^{+}(aq) + NO^{-}_{2}(aq)$

Initially : 0.222 M 0 0.278 M

Change : - x +x +x

Equilibrium : 0.222 M - x x 0.278 M + x

Therefore, dissociation constant for this reaction will be as follows.

$K_{a} = \frac{[H^{+}][NO^{-}_{2}]}{[HNO_{2}]}$

Hence, putting the given values into the above formula as follows.

$K_{a} = \frac{[H^{+}][NO^{-}_{2}]}{[HNO_{2}]}$

$4.50 \times 10^{-4} = \frac{x \times (0.278 + x)}{(0.222 - x)}$

x = 0.00036

As, $[H^{+}]$ is 0.00036 M. Therefore, percentage ionization of $HNO_{2}$ will be calculated as follows.

% ionization of $HNO_{2}$ = $\frac{[H^{+}]}{[HNO_{2}]} \times 100$

= $\frac{0.00036 M}{0.222 M} \times 100$

= 0.16 %

Thus, we can conclude that % ionization of $HNO_{2}$ is 0.16%.

5 0

4 years ago

How many electrons are needed to equal the mass of a proton?

charle [14.2K]

<span>How many electrons are needed to equal the mass of a proton?
</span>
The correct answer is that you need 1836 electron to equal the mass of a proton. This means that a proton is equals to 1836 electron or 1 = 1836. This is the answer to your question. I hope this answer helped you.

5 0

4 years ago

I2 => 2 I I + H2 => H2I H2I + I => 2 HI What is the molecularity of step 2? A. unimolecular B. bimolecular C. termolecu

lianna [129]

Answer : The correct option is, (B) bimolecular

Explanation :

Molecularity : It is defined as the total number of reactant molecules taking part in the balanced equation of a reaction. It is a theoretical concept.

The given chemical reaction are,

Step (1) : $I_2\rightarrow 2I$

Step (2) : $I+H_2\rightarrow H_2I$

Step (3) : $H_2I+I\rightarrow 2HI$

The number of reactants molecules taking part in the balanced equation of a reaction 2 are, $I\text{ and }H_2$ .

In this reaction, 1 'I' molecules reacts with the 1 $H_2$ molecule.

Total number of reactant molecule = 1 + 1 = 2

The molecularity of the reaction is 2 that means, the elementary reaction is bimolecular.

Hence, the correct option is, (B) bimolecular

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3 years ago

In a population of wheat,

andre [41]

Right push is good man

8 0

3 years ago

A sample that contains 4.78 mol of a gas at 251 K has a pressure of 1.19 atm. What is the volume? Answer in units of L.

Y_Kistochka [10]

Answer:
V = 81.86 L

Solution:

Data Given;
P = 1.19 atm

n = 4.78 mol

T = 251 K

Let suppose the gas is acting ideally, then according to Ideal Gas Equation,

P V = n R T

Solving for V,
V = n R T / P

Putting Values,

V = (4.78 mol × 0.0812 L.atm.mol⁻¹.K⁻¹ × 251 K) ÷ 1.19 atm

V = 81.86 L

8 0

4 years ago