All categories

3 years ago

Calculate the [H+] in a solution that has a pH of 10.36

Chemistry

1 answer:

Pavlova-9 [17]3 years ago

5 0

Answer:

[H+] = 4.365x10⁻¹¹

Explanation:

The pH is a measurement widely used in chemistry. Is used in quality control to determine if a product is good for human or pet consumption. The equation to obtain the pH is:

pH = -log [H+]

To solve [H+]:

10^pH = -[H+]

10^-pH = -[H+]

In the problem:

10^-10.36 = -[H+]

You might be interested in

What are valence electrons? how many of a magnesium atom’s 12 electrons are valence electrons?

wlad13 [49]

It has 2 valence electrons.

6 0

3 years ago

If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200 K and then I raise the pressu

mixas84 [53]

Answer:

The answer to your question is V2 = 29.6 l

Explanation:

Data

Pressure 1 = P1 = 12 atm

Volume 1 = V1 = 23 l

Temperature 1 = T1 = 200 °K

Pressure 2 = 14 atm

Volume 2 = V2 = =

Temperature 2 = T2 = 300°K

Process

1.- To solve this problem use the Combine gas law.

P1V1/T1 = P2V2/T2

-Solve for V2

V2 = P1V1T2 / T1P2

2.- Substitution

V2 = (12)(23)(300) / (200)(14)

3.- Simplification

V2 = 82800 / 2800

4.- Result

V2 = 29.6 l

5 0

3 years ago

Comment on whether each of the following is a homogeneous mixture or a heterogeneous mixture: (a) air in a closed bottle, (b) ai

Colt1911 [192]

Explanation:

A mixture in which there is uniform distribution of solute particles into the solvent is known as a homogeneous mixture.

For example, sugar dissolved in water is a homogeneous mixture.

On the other hand, a mixture in which there is uneven distribution of solute particles into the solvent is known as a heterogeneous mixture.

For example, sand present in water is a heterogeneous mixture.

Comment on given situations will be as follows.

(a) Air in a closed bottle - It is a homogeneous mixture because there will be even distribution of other gases that are present in air.

(b) Air over New York City - It is a heterogeneous mixture because there will be presence of some dust particles, fog or smoke into the air. Distribution of all these particles will be uneven. This will make air over New York City heterogeneous in nature.

8 0

3 years ago

Suppose a 2.95 g of potassium iodide is dissolved in 350. mL of a 62.0 m M aqueous solution of silver nitrate. Calculate the fin

STALIN [3.7K]

Answer : The final molarity of iodide anion in the solution is 0.0508 M.

Explanation :

First we have to calculate the moles of $KI$ and $AgNO_3$ .

$\text{Moles of }KI=\frac{\text{Mass of }KI}{\text{Molar mass of }KI}$

Molar mass of KI = 166 g/mole

$\text{Moles of }KI=\frac{2.95g}{166g/mole}=0.0178mole$

and,

$\text{Moles of }AgNO_3=\text{Concentration of }AgNO_3\times \text{Volume of solution}=0.0620M\times 0.350L=0.0217mole$

Now we have to calculate the limiting and excess reagent.

The given chemical reaction is:

$KI+AgNO_3\rightarrow KNO_3+AgI$

From the balanced reaction we conclude that

As, 1 mole of KI react with 1 mole of $AgNO_3$

So, 0.0178 mole of KI react with 0.0178 mole of $AgNO_3$

From this we conclude that, $AgNO_3$ is an excess reagent because the given moles are greater than the required moles and KI is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of $AgI$

From the reaction, we conclude that

As, 1 mole of $KI$ react to give 1 mole of $AgI$

So, 0.0178 moles of $KI$ react to give 0.0178 moles of $AgI$

Thus,

Moles of AgI = Moles of $I^-$ anion = Moles of $Ag^+$ cation = 0.0178 moles

Now we have to calculate the molarity of iodide anion in the solution.

$\text{Concentration of }AgNO_3=\frac{\text{Moles of }AgNO_3}{\text{Volume of solution}}$

$\text{Concentration of }AgNO_3=\frac{0.0178mol}{0.350L}=0.0508M$

Therefore, the final molarity of iodide anion in the solution is 0.0508 M.

3 0

3 years ago

Oxygen gas is collected at a pressure of 123 kPa in a container which has a volume of 10.0L. What temperature must be maintained

Morgarella [4.7K]

Given:

P = 123 kPa
V = 10.0 L
n = 0.500 moles
T = ?

Assume that the gas ideally, thus, we can use the ideal gas equation:

PV = nRT

where R = 0.0821 L atm/mol K

123 kPa * 1 atm/101.325 kPa * 10.0 L = 0.500 moles * 0.0821 Latm/molK * T

solve for T

T = 295.72 K<span />

5 0

3 years ago

Read 2 more answers