sulfamic acid, HSO3NH2, is a strong monoprotic acid that can be used to standardize a strong base :
HSO3NH2(aq)+ KOH(aq) --> KSO3NH2(aq) + H20(l)
A .179g sample of HSO3NH2 required 19.4 mL of an aq soln of KOH for complete reaction. whats the molarity of KOH soln?
This doesn't help
To determine the molarity of the KOH solution, we need to use the balanced chemical equation provided and the mass of HSO3NH2.
The balanced equation is: HSO3NH2(aq) + KOH(aq) -> KSO3NH2(aq) + H2O(l)
From the balanced equation, we can see that the mole ratio between HSO3NH2 and KOH is 1:1. This means that 1 mole of HSO3NH2 reacts with 1 mole of KOH.
First, we need to find the number of moles of HSO3NH2 using its given mass and its molar mass.
The molar mass of HSO3NH2 can be calculated as follows:
H (1 atom) = 1.01 g/mol
S (1 atom) = 32.06 g/mol
O (3 atoms) = 16.00 g/mol x 3 = 48.00 g/mol
N (2 atoms) = 14.01 g/mol x 2 = 28.02 g/mol
The molar mass of HSO3NH2 = 1.01 + 32.06 + 48.00 + 28.02 = 109.09 g/mol
Now, we can calculate the number of moles of HSO3NH2:
Mass of HSO3NH2 = 0.179 g
Number of moles of HSO3NH2 = Mass / Molar mass = 0.179 g / 109.09 g/mol
Next, we need to find the molarity of the KOH solution using the volume of KOH solution.
Volume of KOH solution = 19.4 mL = 0.0194 L
Molarity (M) is defined as moles of solute divided by volume of solution in liters:
Molarity of KOH (M) = Moles of KOH / Volume of KOH solution
Since the mole ratio between HSO3NH2 and KOH is 1:1, the moles of KOH will be the same as the moles of HSO3NH2.
Molarity of KOH = Moles of KOH / Volume of KOH solution
= Moles of HSO3NH2 / Volume of KOH solution
= (0.179 g / 109.09 g/mol) / 0.0194 L
Calculating this expression gives us the molarity of the KOH solution.
To find the molarity of the KOH solution, we need to use the balanced chemical equation and the given data.
The balanced chemical equation for the reaction is:
HSO3NH2(aq) + KOH(aq) --> KSO3NH2(aq) + H2O(l)
From the equation, we can see that the mole ratio between HSO3NH2 and KOH is 1:1. This means that the number of moles of KOH used in the reaction is equal to the number of moles of HSO3NH2.
First, let's find the number of moles of HSO3NH2:
1. Calculate the molar mass of HSO3NH2:
1H (1.007 g/mol) + 1S (32.06 g/mol) + 1O (16.00 g/mol) + 3N (14.01 g/mol) + 2H (1.007 g/mol) = 97.09 g/mol
2. Convert the mass of HSO3NH2 to moles:
mass of HSO3NH2 / molar mass of HSO3NH2 = 0.179 g / 97.09 g/mol = 0.00184 mol
Since the molar ratio between HSO3NH2 and KOH is 1:1, the number of moles of KOH used in the reaction is also 0.00184 mol.
Next, we need to calculate the volume of the KOH solution. We are given that it took 19.4 mL (milliliters) of the KOH solution to react completely with the HSO3NH2.
To find the molarity, we need to convert mL to L:
volume of KOH solution = 19.4 mL / 1000 (to convert mL to L) = 0.0194 L
Now, we can calculate the molarity (M) of the KOH solution:
Molarity (M) = moles of solute / volume of solution (in L)
Molarity (KOH) = 0.00184 mol / 0.0194 L ≈ 0.095 M
Therefore, the molarity of the KOH solution is approximately 0.095 M.
1. Convert 0.179 g sulfamic acid to moles. moles = grams/molar mass.
2. Using the coefficients in the balanced equation, convert moles sulfamic acid to moles KOH.
3. Now use the definition of molarity = moles/L