What is the pH of the resulting solution when 25.0mL of 0.100 HNO3(aq)are reacted with 20.0 mL NaOH(aq)? Is the resulting solution acidic or basic in nature?
To find the pH of the resulting solution, you need to determine the concentration of H+ ions in the solution after the reaction between HNO3(aq) and NaOH(aq).
Step 1: Calculate the moles of HNO3 and NaOH used in the reaction.
Moles of HNO3 = volume (in liters) x molarity = 0.025 L x 0.100 mol/L
Moles of NaOH = volume (in liters) x molarity = 0.020 L x molarity (assume it is 1.00 mol/L in this case, as it is not given)
Step 2: Determine which reactant is in excess.
To do this, compare the number of moles of each reactant. In this case, HNO3 and NaOH react in a 1:1 ratio, so compare the number of moles directly. If HNO3 is in excess, the remaining moles of HNO3 will react with water to produce H3O+ ions, making the resulting solution acidic. If NaOH is in excess, the remaining moles of NaOH will react with water to produce OH- ions, making the solution basic.
Step 3: Calculate the moles of H+ or OH- ions produced by the excess reactant.
Assuming HNO3 is in excess, the remaining moles of HNO3 will react with water to produce H3O+ ions. Since one molecule of HNO3 produces one H3O+ ion, the moles of H3O+ ions produced would be equal to the moles of HNO3 remaining.
Step 4: Calculate the concentration of H+ ions (or OH- ions) in the solution.
The concentration of H+ ions (or OH- ions) can be calculated by dividing the moles of H+ ions (or OH- ions) by the total volume of the resulting solution, which is the sum of the volumes of the reactants used.
Step 5: Calculate the pH of the resulting solution.
pH is calculated using the formula pH = -log[H+], where [H+] is the concentration of H+ ions in moles per liter. If the concentration of H+ ions is known, you can substitute it into the formula to determine the pH.
Based on the information provided, you can use the steps outlined above to calculate the pH of the resulting solution and determine if it is acidic or basic in nature.
To determine the pH of the resulting solution, we can first calculate the amount of HNO3 and NaOH that reacts.
Step 1: Calculate the amount of HNO3 in moles.
Given volume of HNO3 = 25.0 mL
Concentration of HNO3 = 0.100 M
Moles of HNO3 = (volume x concentration) / 1000
= (25.0 mL x 0.100 mol/L) / 1000
= 0.0025 mol
Step 2: Calculate the amount of NaOH in moles.
Given volume of NaOH = 20.0 mL
Concentration of NaOH = unknown
In order to continue, we need to know the concentration of NaOH.
Step 3: Determine the limiting reactant.
The reacting ratio between HNO3 and NaOH is 1:1. Since we have equal volumes of both solutions, the limiting reactant will be the one with fewer moles.
In this case, HNO3 has 0.0025 mol, so NaOH should also have 0.0025 mol.
Step 4: Calculate the concentration of NaOH.
Moles of NaOH = 0.0025 mol
Volume of NaOH = 20.0 mL
Concentration of NaOH = (moles / volume) x 1000
= (0.0025 mol / 20.0 mL) x 1000
= 0.125 M
Step 5: Determine the resulting solution's pH.
Since equal amounts of a strong acid (HNO3) and a strong base (NaOH) react, they will completely neutralize each other, leaving only water and a neutral pH of 7.
Therefore, the resulting solution will be neutral with a pH of 7.