Answer:
pH = 2
A 0.010 M solution of hydrochloric acid, HCl, has a molarity of 0.010 M. This means that [H+] = 1 x 10-2 M. The pH of this aqueous solution of H+ ions is pH = 2
hope this helps :3
Answer:
7.52 x 10²³ molecules N
Explanation:
multiply 1.25 mol of N2 by Avogadro's Number
Answer:
The number before any molecular formula applies to the entire formula. So here you have five molecules of water with two hydrogen atoms and one oxygen atom per molecule. Thus you have ten hydrogen atoms and five oxygen atoms in total.
D. Itd be 4+. Hope it helps
Answer:
10.96
Explanation:
<em>A solution is prepared at 25 °C that is initially 0.14 M in diethylamine, a weak base with Kb = 1.3 × 10⁻³, and 0.20 M in diethylammonium chloride. Calculate the pH of the solution. Round your answer to 2 decimal places.</em>
Step 1: Calculate the pOH of the solution
Diethylamine is a weak base and diethylammonium (from diethylammonium chloride) its conjugate acid. Thus, they form a buffer system. We can calculate the pOH of this buffer system using the Henderson-Hasselbach's equation.
pOH = pKb + log [acid]/[base]
pOH = -log 1.3 × 10⁻³ + log 0.20 M/0.14 M
pOH = 3.04
Step 2: Calculate the pH of the solution
We will use the following expression.
pH + pOH = 14
pH = 14 - pOH = 14 -3.04 = 10.96
