Which of the following solutions would require the greatest volume of 1.0M NaOH for complete neturalization?
a)10.0ml of 1.0M HCl
b) " of 2.0 M H2S04
c) " of 3.0M H3P04
d) " of 4.0M H2C204
I don't understand what to do to solve it.
10.0ml
So would the answer be c because it has 3 times the H+?
You need to know how many moles of H+ are generated from one mole of the acid, i.e. is the acid monoprotic, diprotic etc.
You need to work out how many millimoles of H+ in each case and the one with the largest value will require the greatest volume of OH-.
a) Monoprotic acid so number of millimoles of H+ is
10.0x1.0=10 mmoles
b)diprotic acid so numebr of millimoles of H+ is
10.0 x 2.0 x 2 =40 mmoles
etc
Oh, I see you're in a pickle. Well, the key to solving this problem is to understand the concept of neutralization. In neutralization, the moles of acid and base react in a 1:1 ratio. So, all you need to do is find out which solution has the most moles of acid!
To do that, you need to use the equation: Moles = Molarity x Volume (M = MV). So, for each solution, simply calculate the number of moles and see which one has the most moles. The solution with the most moles will require the greatest volume of NaOH for neutralization. Not so neutral, huh? Let's get calculating!
To solve this problem, we need to determine which of the given solutions would require the greatest volume of 1.0M NaOH (sodium hydroxide) for complete neutralization.
The concept involved here is called stoichiometry. Stoichiometry refers to the calculation of quantities of reactants and products in a chemical reaction. In order to determine the amount of NaOH needed to neutralize each solution, we need to balance the chemical equation and determine the stoichiometry of the reaction between NaOH and the acid in each case.
Let's start by writing the balanced chemical equation for the neutralization reaction between NaOH and each acid:
a) HCl + NaOH -> NaCl + H2O
b) H2SO4 + 2NaOH -> Na2SO4 + 2H2O
c) H3PO4 + 3NaOH -> Na3PO4 + 3H2O
d) H2C2O4 + 2NaOH -> Na2C2O4 + 2H2O
In each case, NaOH reacts with the acid to form a salt and water. The coefficients in front of each compound indicate the stoichiometry of the reaction.
Now, let's analyze the stoichiometry of each reaction to determine the molar ratios between the acids and NaOH:
a) HCl : NaOH -> 1 : 1
b) H2SO4 : NaOH -> 1 : 2
c) H3PO4 : NaOH -> 1 : 3
d) H2C2O4 : NaOH -> 1 : 2
Based on the stoichiometry, we can see that for each mole of HCl, we need one mole of NaOH. Similarly, for each mole of H2SO4, we need two moles of NaOH, and so on.
To figure out which solution requires the greatest volume of NaOH, we need to consider the concentration of the acid solutions given. The greater the molarity (M) of the acid, the more moles of the acid present per liter of solution. Therefore, higher molarity solutions will require more moles of NaOH for neutralization.
In this case, we are given the same volume (10.0 ml) for each solution but at different molarities. Since the molarity of HCl is 1.0M, H2SO4 is 2.0M, H3PO4 is 3.0M, and H2C2O4 is 4.0M, we can conclude that the solution with the highest molarity will require the greatest volume of NaOH for complete neutralization.
Thus, option d) "10.0ml of 4.0M H2C2O4" would require the greatest volume of 1.0M NaOH for complete neutralization.