The number of hydrogen ions in 4.9g of tetraoxosulphate(iv)acid is what?
Show workings bit by bit
To solve this problem, we need to use the formula for calculating the number of moles of a substance:
moles = mass ÷ molar mass
Then, we can use the balanced equation for the dissociation of tetraoxosulphate(iv) acid to calculate the number of hydrogen ions:
H2SO4 → 2H+ + SO4 2-
From the equation, we can see that for each molecule of H2SO4 that dissociates, two hydrogen ions are formed. Therefore, we need to multiply the number of moles of H2SO4 by 2 to get the number of hydrogen ions.
Step 1: Calculate the molar mass of H2SO4
H = 1.01 x 2 = 2.02
S = 32.07
O = 16.00 x 4 = 64.00
Total molar mass = 2.02 + 32.07 + 64.00 = 98.09 g/mol
Step 2: Calculate the number of moles of H2SO4
moles = mass ÷ molar mass
moles = 4.9 g ÷ 98.09 g/mol
moles = 0.0499 mol
Step 3: Calculate the number of hydrogen ions
number of H+ ions = 2 x moles of H2SO4
number of H+ ions = 2 x 0.0499 mol
number of H+ ions = 0.0998 mol
Step 4: Convert the number of moles of H+ ions to number of ions
Number of ions = Avogadro's number x number of moles
Number of ions = 6.022 x 10^23 ions/mol x 0.0998 mol
Number of ions = 6.011 x 10^22 ions
Therefore, the number of hydrogen ions in 4.9g of tetraoxosulphate(iv)acid is 6.011 x 10^22 ions.