If you have 45.6mL of a liquid and its

Enter your answer in the provided box. calculate the ph of a 0. 39 m ch3cooli solution. (ka for acetic acid = 1. 8 × 10−5. )

loris [4]

The pH of the solution is the negative logarithm of a proton or the hydrogen ion concentration. The pH of 0.39 M acetic acid solution (CH₃COONa) is 2.58.

The pH has been said to be the hydrogen ion concentration that can also be given by the pOH.

Given,

The acid dissociation constant Ka = 1.8 × 10⁻⁵

Concentration of acetic acid (C) = 0.39 M

The hydrogen ion concentration from Ka and molar concentration are calculated as:

H⁺ = √ Ka × C

= √1.8 × 10⁻⁵ × 0.39

= √0.00000702

= 0.0026

Now, pH from hydrogen ion is calculated as,

pH = - log [H⁺]

= - log [0.0026]

= 2.58

Therefore, the pH of acetic acid is 2.58.

Learn more about pH here:

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6 0

2 years ago

The formation constant* of [M(CN) 4 ]2− is 7.70 × 10 16 , where M is a generic metal. A 0.150 mole quantity of M(NO3)2 is added

iogann1982 [59]

Answer:

0 M.

Explanation:

Hello,

In this case, the undergoing reaction is:

$M(NO_3)_2+NaCN\leftrightarrow [M(CN)_4]^{-2}+NaNO_3$

Nonetheless, it only matters the reaction forming the given complex:

$M^{+2}+4CN^-\leftrightarrow [M(CN)_4]^{-2}$

In such a way, the formation constant turns out:

$K_F=\frac{[[M(CN)_4]^{-2}]_{eq}}{[M^{+2}]_{eq}[CN^{-}]_{eq}^4}$

Now, one could assume that the initial concentrations of the ions equals the original compounds concentrations:

$[M^{+2}]_0=0.150M;[CN^-]_0=0.820M$

In such a way, we modify the formation constant in terms of the change $x$ due to the reaction progress:

$K_F=\frac{x}{(0.150-x)(0.820-x)^4}=7.70x10^{16}$

Now, solving for $x$ :

$x_1=0.15M\\x_2=0.82M$

The feasible solution is 0.15M which will lead to an equilibrium concentration of M⁺² of 0M

$[M^{+2}]_{eq}=0.15M-0.15M=0M$

This fact has sense since the formation constant is very large.

Best regards.

3 0

3 years ago

Someone help me please i’ll give brainly

quester [9]

Answer:

b

Explanation:

i looked it up on Google

4 0

3 years ago

The figure shows the skeletal structure in line-angle (line-bond) mode of 2,5-dimethylhexa-1,4-diene. Identify the number of

deff fn [24]

Answer:

There are 22 hydrogen in 2,3,3,5-tetramethylhexane (C10H22)

From the left to the right of the skeletal structure:

1st Main Carbon = 3 hydrogen

2nd Main Carbon = 1 hydrogen

1st Branch Carbon = 3 hydrogen

3rd Main Carbon = 2 hydrogen

2nd Branch Carbon = 3 hydrogen

3rd Branch Carbon = 3 hydrogen

4th Main Carbon = 0 hydrogen

4th Branch Carbon = 3 hydrogen

5th Main Carbon = 1 hydrogen

6th Main Carbon = 3 hydrogen

Total = 22 hydrogen

Explanation:

This is the skeletal formula for 2,3,3,5-tetramethylhexane - the 2D chemical structure. It is an organic compound. The carbon atoms in the structure are known as the carbon backbone. The hydrogen atoms are linked to the carbon backbone. This provides each carbon atom with four bonds.

Explanation:

5 0

3 years ago

What is the pressure in atm of 0.47mol of a gas in a 1.7L container at 276K?

polet [3.4K]

The answer is 1. A sample of 0.50 moles of gas is placed in a container of volume of 2.5 L. What is the pressure of the gas in torr if the gas is at 25oC? P = 4.89 atm = 3719 torr

2. A sample of gas is placed in a container at 25oC and 2 atm of pressure. If the temperature is raised to 50oC, what is the new pressure? P = 2.17 atm

3. At 1 atm of pressure water boils at 100oC, if the sample was placed under 2 atm of pressure, what would be the temperature? (This would be like a pressure cooker).
T = 746 K = 473oC = 883oF

4. At what temperature would water boil if the pressure is 600 torr? (Use information from problem 3: this shows why food doesn't cook well at higher elevations)
T = 294 K = 21.5oC = 70.7oF

5. Calculate the volume of 40.6 g of F2 at STP. V = 23.9 L

6. A sample of 2.0 moles of hydrogen gas is placed in a container with a volume of 10.4 L. What is the pressure of the gas in torr if the gas is at 25oC? P = 4.70 atm = 3576

7. The tire pressure is 32 psi. What is the pressure in torr if 1 atm = 14.7 psi?
P = 1654 torr

8. A gas is placed in a balloon with a volume of 3.0 L at 28oC and 900 torr. What would be the new volume for the gas if placed under STP? V = 3.2 L

9. How many moles of gas would occupy a volume of 14 L at a pressure of 700 torr and a temperature of 30oC? n = 0.52 mol

10. Calculate the volume of 24.0 g of HCl at STP. V = 14.8 L

11. What is the volume of one mole of acetylene gas at STP? V =22.414 L

12. What is the volume of 0.75 mol of gas at 72oC and 2 atm? V = 10.6 L

13. After eating beans, a student collects a sample of gas at 0.97 atm and 26oC which occupies a volume of 3.5 L, calculate its volume at STP. V = 3.1 L

14. Ammonia (NH3) is placed in 1.5 L flask at 25oC. If the pressure of the gas is 0.899 atm, what is the density? d = 0.626 g/L

15. A mixture of Ar and CO gases is collected over water at 28oC and an atmospheric pressure of 1.05 atm. If the partial pressure of Ar is 600 torr, what is the partial pressure of CO? (vapor pressure of water at 28oC is 28.3 mmHg) PCO = 0.223 atm

16. Determine the partial pressures of each of the gases in the following mixture: 17.04 g NH3, 40.36 g Ne and 19.00 g F2. The gases are at 1.5 atm of pressure.
PNH3 = 0.428 atm; PNe = 0.857 atm; PF2 = 0.2124 atm

17. Potassium chlorate decomposes under heat as follows:

2 KClO3 (s) -------> 2 KCl (s) + 3 O2 (g)

The oxygen gas is collected over water at 25oC. The volume of gas is 560 mL measured at 1 atm. Calculate the number of grams of KClO3 used in the reaction. (vapor pressure of water = 0.0313 atm) nO2 = 0.022 mol; 1.81 g KClO3

5 0

2 years ago