A student is asked to make a solution of sodium hydroxide by dissolving an unknown mass of pellets in 250cm3 of water. 25cm3 of solution is then titrated against a standard solution of hydrochloric acid (0.50M) using a suitable indicator to identify the neutralization point. What are the number of moles of sodium hydroxide in 25.0cm3 and the 250cm3 solution. Volume of sodium hydroxide =25.05cm3, moles of HCl=0.00125 moles

Using a value of ksp = 1.8 x 10-2 for the reaction pbcl2 pb+2(aq) + 2cl -(aq). if the value of ksp was determined to be only 1.2 x 10-2: too much solid has dissolved. additional precipitate is forming. the solution is unsaturated. the ions are now combining to reduce their concentrations.

Define dew point. i am writing this part to be able to ask the question

The lattice enthalpy (formation of ionic solid from ions in the gas phase) for agcl(s) is -916 kj/mol and the hydration enthalpy (dissolution of gaseous ions into water) is -850 kj/mol. how much heat (in joules) is involved in forming 1l of saturated agcl solution (1.8 × 10-4 g / 100 ml water) by dissolving agcl(s)? assume solution volume does not change much upon dissolution. the equations are given below. ag+(g) + cl−(g) æ agcl(s)