Aqueous sulfurous acid (H2SO3) was made by dissolving .200L of sulfur dioxide gas at 19 degrees C and 745 mmHg in water to yield 500mL of solution. the acid solution required 12mL of sodium hydroxide solution to reach the titration end point. what was the molarity of the sodium hydroxide solution?
I wonder WHICH titration end point was reached.
2NaOH + H2SO3 ==> Na2SO3 + 2H2O
moles NaOH = M x L = ??
Use the coefficients in the balanced equation to convert moles NaOH to moles H2SO3.
M = moles/L.
To find the molarity of the sodium hydroxide (NaOH) solution, we need to first determine the number of moles of NaOH used in the titration.
Step 1: Calculate the number of moles of H2SO3
To do this, we can use the ideal gas law to find the number of moles of sulfur dioxide (SO2) gas used in the reaction:
PV = nRT
P = pressure in atm = 745 mmHg = 0.982 atm (converting mmHg to atm)
V = volume in liters = 0.200 L
n = number of moles
R = ideal gas constant = 0.0821 L·atm/(mol·K)
T = temperature in Kelvin = 19 °C + 273.15 = 292.15 K
Using the ideal gas law equation, we can solve for n:
n = PV / RT
n = (0.982 atm * 0.200 L) / (0.0821 L·atm/(mol·K) * 292.15 K)
Step 2: Calculate the molarity of H2SO3
Since the equation for the reaction between H2SO3 and NaOH is 1:1, the moles of NaOH used will be equal to the moles of H2SO3 used. Therefore, we can use the moles of H2SO3 to calculate its molarity.
Molarity = Moles / Volume
Volume = 500 mL = 0.500 L
Molarity = n / V
Molarity = (moles of H2SO3) / 0.500 L
Step 3: Calculate the molarity of NaOH
Since the molarity of H2SO3 is equal to the molarity of NaOH, we can use the volume and molarity of NaOH to calculate its molarity.
Volume = 12 mL = 0.012 L
Molarity of NaOH = Molarity of H2SO3 = moles of H2SO3 / 0.012 L
Now, we can substitute the values and calculate the molarity of NaOH.