What is the H+ ion concentration of this solution?
A solution is made by dissolving 0.0112 g KOH in enough water to make 1.0 liter of solution. What is the H+ ion concentration of this solution?
a. ) 2.0 x 10-3 M
b. ) 8.0 x 10-2 M
c. ) 1.2 x 10-13 M
d. ) 5.0 x 10-11 M
e. ) 5.0 x 10-12 M
Convert g KOH to mols KOH.
M = mols/L of solution.
(OH^-) same as (KOH)
(H^+)(OH^-) = Kw = 1 x 10^-14
You know (OH^-) and Kw; solve for (H^+). The answer is about 10^-11 if I didn't make a mistake but you will need to work it out to get the exact answer.
Well, let's evaluate this problem together. First, we need to find the moles of KOH in the solution. The molar mass of KOH is 56.11 g/mol, so the number of moles can be calculated by dividing the mass (0.0112 g) by the molar mass.
Now, we have the number of moles of KOH in 1.0 liter of solution. Remember that KOH is a strong base that dissociates in water to form K+ and OH- ions. Since OH- is a hydroxide ion, we must find the concentration of OH- ions and convert it to the H+ ion concentration (since we are interested in the concentration of H+).
In this case, the concentration of OH- ions is equal to the moles of KOH divided by the volume of the solution (1.0 L). This concentration can be converted to the H+ ion concentration using the equation Kw = [H+][OH-]. Since water is neutral, the H+ and OH- ions concentrations are equal, so we can substitute the [OH-] concentration with the concentration of OH- ions obtained from the previous step.
To calculate the H+ ion concentration, we need to know the value of Kw, the ion product of water, which is equal to 1.0 x 10^-14. Then, we can solve the equation Kw = [H+][OH-] for [H+].
Now, let's make a funny chemistry joke: Why do chemists like nitrates so much? Because they are cheaper than day rates!
Alright, back to the question. After substituting the value of Kw and the [OH-] concentration, we can solve for the [H+] concentration. Once we calculate that, we can compare it to the answer choices given.
So, let's start crunching those numbers! You got this!
To find the H+ ion concentration of the solution, we need to determine the concentration of OH- ions first, since KOH dissociates into K+ and OH- ions.
Step 1: Determine the moles of KOH.
molar mass of KOH = 39.10 g/mol (K) + 16.00 g/mol (O) + 1.01 g/mol (H) = 56.11 g/mol
moles of KOH = 0.0112 g / 56.11 g/mol = 1.998 x 10^-4 mol
Step 2: Determine the concentration of KOH.
concentration = moles/volume
volume of solution = 1.0 L
concentration of KOH = 1.998 x 10^-4 mol / 1.0 L = 1.998 x 10^-4 M
Step 3: Determine the concentration of OH- ions.
Since one mole of KOH produces one mole of OH-, the concentration of OH- ions is also 1.998 x 10^-4 M.
Step 4: Determine the concentration of H+ ions.
Since water is a neutral substance, the concentration of H+ ions is equal to the concentration of OH- ions.
Therefore, the H+ ion concentration of the solution is 1.998 x 10^-4 M.
None of the given answer choices matches the calculated value of 1.998 x 10^-4 M.
To find the H+ ion concentration of the solution, we need to determine the concentration of hydroxide ions (OH-) first. The KOH (potassium hydroxide) dissociates in water to form potassium ions (K+) and hydroxide ions (OH-). The balanced equation for this dissociation is:
KOH -> K+ + OH-
We are given that 0.0112 g of KOH is dissolved in 1.0 liter of solution. First, let's calculate the moles of KOH:
Molar mass of KOH = atomic mass of K + atomic mass of O + atomic mass of H
= (39.10 g/mol) + (16.00 g/mol) + (1.01 g/mol)
= 56.11 g/mol
Moles of KOH = mass of KOH / molar mass of KOH
= 0.0112 g / 56.11 g/mol
≈ 1.995 x 10^-4 mol
Since the molar ratio between KOH and OH- is 1:1, the concentration of OH- ions in the solution is equal to the concentration of KOH. Therefore, we have:
OH- ion concentration = moles of KOH / volume of solution
= 1.995 x 10^-4 mol / 1.0 L
= 1.995 x 10^-4 M
In a neutral solution, the concentration of H+ ions is equal to the concentration of OH- ions (due to water autoprotolysis). Therefore, the H+ ion concentration in this solution is also 1.995 x 10^-4 M.
However, none of the given answer choices match this result. Therefore, it seems that there might be an error or omission in the question or answer choices provided.