If 250ml of Ba(OH)2 is unknown concerntration with methyl red indicator present is tritrated with [0.325M]HNO3, the yellow solution turns red after 36.4 ml of the HNO3 is added. What is the molarity of Ba(OH)2
Write and balance the equation.
Calculate moles HNO3. moles = M x L.
Convert moles HNO3 to moles Ba(OH)2 using the coefficients in the balanced equation. Finally, use M = moles/L to calculate molarity.
To determine the molarity of Ba(OH)2, we can use the concept of titration. In this scenario, Ba(OH)2 is being titrated with HNO3, and the methyl red indicator is being used to determine the endpoint of the titration.
First, let's set up the balanced chemical equation for the reaction between Ba(OH)2 and HNO3:
Ba(OH)2 + 2HNO3 -> Ba(NO3)2 + 2H2O
From the balanced chemical equation, we can see that the ratio of Ba(OH)2 to HNO3 is 1:2. This means that every 1 mole of Ba(OH)2 will react with 2 moles of HNO3.
Next, we can determine the number of moles of HNO3 used in the titration. We know that the concentration of the HNO3 solution is 0.325M and the volume used is 36.4 ml (0.0364 L). To calculate the number of moles, we can use the formula:
moles = concentration (M) x volume (L)
moles of HNO3 = 0.325M x 0.0364L = 0.01181 moles
Since the ratio of Ba(OH)2 to HNO3 is 1:2, the number of moles of Ba(OH)2 used in the titration is half of the moles of HNO3:
moles of Ba(OH)2 = 0.01181 moles / 2 = 0.005905 moles
Now, we can determine the molarity of Ba(OH)2 by rearranging the formula:
molarity = moles / volume (L)
Since we know that the volume used for Ba(OH)2 solution is 250 ml (0.250 L), we can plug in the values:
molarity of Ba(OH)2 = 0.005905 moles / 0.250 L = 0.02362 M
Therefore, the molarity of the Ba(OH)2 solution is 0.02362 M.