Solubility of CaSO_4 =" 0.21g"/"100ml"CaSO4= 0.21g100ml
Amount of water required to dissolve 68g of CaSO_4CaSO4
= "100ml"/"0.21g" *68g=32380.952380952380952380952380952L100ml0.21g⋅68g=32380.952380952380952380952380952L
This means there is 32380.9524L of water and 68g of CaSO_4CaSO4
No. of ions in 68g of calcium sulphate in water
No. of moles in 68g of CaSO_4CaSO4
"68g"/"136.14g/mol" = 0.49948582341"moles"68g136.14g/mol=0.49948582341moles
CaSO_4 rightleftharpoons Ca^(+2) + SO4^2-CaSO4⇌Ca+2+SO42−
No. of Ca^(+2)Ca+2 ions
0.49948582341"moles" * 1/1 * "6.022 * 10^23Ca(+2)ions"/"1mol Ca"0.49948582341moles⋅11⋅6.022 * 10^23Ca(+2)ions1mol Ca
= 300790362857502000000000 "ions of Ca"=300790362857502000000000ions of Ca
This there are also 300790362857502000000000 ions of SO4^-2SO4−2
No. of ions in 32380.952380952380952380952380952L
"32380.952380952380952380952380952L * 1000g = "32380952.380952380952380952380952g = 32380952.4g("rounded off)32380.952380952380952380952380952L * 1000g = 32380952.380952380952380952380952g=32380952.4g(roundedoff)
Moles = 32380952.4g/18.01528g
= 1 797415.99 moles
H_2O rightleftharpoons H^+ + OH^-H2O⇌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"1797415.99248mol⋅1mol H+1molH2O⋅6.023⋅1023molH+mol1molH2=1082403910671456000000000000000ions
total ions
2(1082403910671456 * 10 ^ 15 ) + 2(300790362857502000000000) 2(1082403910671456⋅1015)+2(300790362857502000000000)= calculate yourself
