Solubility of #CaSO_4 =" 0.21g"/"100ml"#
Amount of water required to dissolve 68g of #CaSO_4#
=# "100ml"/"0.21g" *68g=32380.952380952380952380952380952L#
This means there is 32380.9524L of water and 68g of #CaSO_4#
No. of ions in 68g of calcium sulphate in water
No. of moles in 68g of #CaSO_4#
#"68g"/"136.14g/mol" = 0.49948582341"moles"#
#CaSO_4 rightleftharpoons Ca^(+2) + SO4^2-#
No. of #Ca^(+2)# ions
#0.49948582341"moles" * 1/1 * "6.022 * 10^23Ca(+2)ions"/"1mol Ca"#
#= 300790362857502000000000 "ions of Ca"#
This there are also 300790362857502000000000 ions of #SO4^-2#
No. of ions in 32380.952380952380952380952380952L
#"32380.952380952380952380952380952L * 1000g = "32380952.380952380952380952380952g = 32380952.4g("rounded off)#
Moles = 32380952.4g/18.01528g
= 1 797415.99 moles
#H_2O rightleftharpoons H^+ + OH^-#
Number of H^+ ions = OH^- ions
#"1797415.99248mol" * "1mol H+"/"1molH2O" * (6.023 * 10^23"mol" H^+ "mol")/(1 "mol"H_2) = 1082403910671456000000000000000"ions"#
total ions
#2(1082403910671456 * 10 ^ 15 ) + 2(300790362857502000000000) #= calculate yourself
