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2 years ago

The pH of a solution is 2.0. Which statement is correct?

Chemistry

1 answer:

mamaluj [8]2 years ago

4 0

Answer:

pH + pOH = 14, [H₃0⁺] [0H⁻] = 10⁻¹⁴

Explanation:

When it comes to questions involving pH, the equations used are;

[H₃0⁺] [0H⁻] = 10⁻¹⁴

This equation shows the concentration of hydroxonium ions alongside that of the hydroxide ions.

pH + pOH = 14

If the value of either the pH of the pOH is know,one can calculate the value of the other using this equation.

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Calculate either [ H 3 O + ] or [ OH − ] for each of the solutions.

STALIN [3.7K]

Answer: Solution A : $[H_3O^+]=0.300\times 10^{-7}M$

Solution B : $[OH^-]=0.107\times 10^{-5}M$

Solution C : $[OH^-]=0.177\times 10^{-10}M$

Explanation:

pH or pOH is the measure of acidity or alkalinity of a solution.

pH is calculated by taking negative logarithm of hydrogen ion concentration and pOH is calculated by taking negative logarithm of hydroxide ion concentration.

$pH=-\log[H_3O^+]$

$pOH=-log[OH^-}$

$pH+pOH=14$

$[H_3O^+][OH^-]=10^{-14}$

a. Solution A: $[OH^-]=3.33\times 10^{-7}M$

$[H_3O^+]=\frac{10^{-14}}{3.33\times 10^{-7}}=0.300\times 10^{-7}M$

b. Solution B : $[H_3O^+]=9.33\times 10^{-9}M$

$[OH^-]=\frac{10^{-14}}{9.33\times 10^{-9}}=0.107\times 10^{-5}M$

c. Solution C : $[H_3O^+]=5.65\times 10^{-4}M$

$[OH^-]=\frac{10^{-14}}{5.65\times 10^{-4}}=0.177\times 10^{-10}M$

7 0

2 years ago

Consider the reaction of A(g) + B(g) + C(g) => D(g) for whichthe following data were obtained:

AveGali [126]

Answer:

rate= k[A]²[B]²[C]

Explanation:

When concentration of A is increased two times ,keeping other's concentration constant , rate of reaction becomes 4 times .

So rate is proportional to [A]²

When concentration of B is increased two times , keeping other's concentration constant,rate of reaction becomes 4 times.

So rate is proportional to [B]²

When concentration of C is increased two times , keeping other's concentration constant, rate of reaction becomes 2 times.

So rate is proportional to [C]

So rate= k[A]²[B]²[C]

5 0

3 years ago

How many grams of magnesium oxide are needed to produce 264g of magnesium hydroxide

Archy [21]

If its one part magnesium and two parts hydroxide id say 88g of magnesium

3 0

3 years ago

A sample of 3.62 moles of diphosphorous trioxide is

Sindrei [870]

$H_3PO_3$ $2H_3PO_3$ $2H_3PO_3$ $P_2O_3$ Answer:

Explanation:

This question is about stoichiometry. From the balanced equation $P_2O_3 + 3H_2O$ ⇒ $2H_3PO_3$ , we see that 3 moles of water is needed to react with 1 mole of $P_2O_3$ .

This means that, to fully react 3.62 moles of $P_2O_3$ , we would need 3*3.62 or 10.86 moles of water. However, we only have 6.31 moles, so water is the limiting reactant.

Since 3 moles of water react with 1 mole of $P_2O_3$ , 6.31 moles of water can fully react with 6.31÷3 or 2.1033 moles of $P_2O_3$ .

From the balanced equation, we see that every mole of $P_2O_3$ reacted gets you 2 moles of $2H_3PO_3$ . Therefore, 2.1033 moles of $P_2O_3$ would give you approximately 4.21 moles of $H_3PO_3$ .

5 0

2 years ago

Answer the following questions:

Vera_Pavlovna [14]

Answer:

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4 0

2 years ago

Read 2 more answers