Question

Calculate the pH of a solution obtained by mixing 489 mL of 0.17 M hydrochloric acid with 311 mL of 2.1 x 10-2 M lithium hydroxide. Assume the combined volume is the sum of the two original volumes. pH =

Answer 1

Similarly moles of Lion Qua Solve Given; Volume of HCl solution = 489mL Concentration of HCl = 0.17M. Volume of liol 311 m L; Concentration of liohs 201410217- soi moles of concentration of HCl X volume of = 0.17 MX 489mL HCl HCI 83-13 mmol. concentration ofx volume of = 2.1x1024 x 311 mL lioh Liol = 6-531 mmol Reaction is HCl + Licht - Lici + to Herei moles of Ht im Hecl> moles of Oli in liol Thus, moles of Ht in hcl reacted is; Total volume ofter =4.89 m1t3'll ml moles of it in HCl = moles of h fooml -moles of of in Lich remain in HCl 83-13 mmol 6-531 mmol. = 76-599 mmol. mixing = f = CS Scanned with CamScanner

So; Concentration of Ht in tel = moles of Htin Hei demaining Total volume of ter mining 76-599 mmol = 0 - 09547 2oo nL Ther; pH = -log (concentration of HP) ple-log (0:0957) = 1.019 Hence; ph solution 1.02. of a CS Scanned with CamScanner