50.0 mL of a 0.20 mol/L HCl reacts with 60.0 mL of 0.15 mol/L NaOH. What is the pH of the final solution?
I tried writing out the equation:
HCl + NaOH = Cl + NaH2O
Now, I am not sure of NaH2O is the right product or not..
However, I am still confused on how I can ifnd the final pH.
yes it is had the same hw
Oh okay thanks!
But could you take me throught the steps to get to the final answer please? or at least lead me in the right direction ?
ok did you happen to get 0.082 mol/L or 0.164 mol/L as possible concentrations?
Can anyone please help me out here?
I believe both of you are confused.
HCl + NaOH ==> NaOH + H2O
mols HCl = M x L = ?
mols NaOH = M x L = ?
You go through the math above and find HCl is greater mols than NaOH by 0.001
Then (HCl) = mols/L = 0.001/0.110
To find the pH of the final solution, you first need to determine the moles of HCl and NaOH that react with each other and then calculate the concentration of the remaining reactants and products.
Let's start by calculating the moles of HCl and NaOH. We know the volume (in mL) and concentration (in mol/L) of each solution. In order to calculate the moles, we need to convert the volume to liters:
Moles of HCl = volume of HCl (in L) × concentration of HCl (in mol/L)
= 50.0 mL ÷ 1000 mL/L × 0.20 mol/L
= 0.010 mol
Moles of NaOH = volume of NaOH (in L) × concentration of NaOH (in mol/L)
= 60.0 mL ÷ 1000 mL/L × 0.15 mol/L
= 0.009 mol
Based on the balanced chemical equation you wrote, the reaction between HCl and NaOH produces NaCl and H2O.
Therefore, the moles of NaCl and H2O formed will be equal to the moles of HCl and NaOH used in the reaction.
Now, let's calculate the concentration of NaCl in the final solution. To do this, we need to find the total volume of the solution after the reaction.
Total volume of the solution = volume of HCl + volume of NaOH
= 50.0 mL + 60.0 mL
= 110.0 mL
Now, let's convert this volume to liters:
Total volume of solution (in L) = 110.0 mL ÷ 1000 mL/L
= 0.110 L
Concentration of NaCl = moles of NaCl / total volume of solution
Since the moles of NaCl is equal to the moles of HCl used in the reaction, which is 0.010 mol, we can substitute this value into the equation:
Concentration of NaCl = 0.010 mol / 0.110 L
= 0.091 mol/L
To find the pH of the solution, we need to determine the concentration of H3O+ (hydronium ions), as it is a measure of acidity.
Since NaCl is a strong electrolyte, it dissociates completely, resulting in the formation of Cl- ions and H3O+ ions:
NaCl → Na+ + Cl-
Now, the concentration of H3O+ ions is equal to the concentration of Cl- ions. Therefore, the concentration of H3O+ ions is 0.091 mol/L.
pH is defined as the negative logarithm (base 10) of the concentration of H3O+ ions:
pH = -log10[H3O+]
Substituting the concentration of H3O+ ions into the equation:
pH = -log10(0.091)
≈ 1.04
Therefore, the pH of the final solution is approximately 1.04.