Many metal ions are precipitated from solution by the sulfide ion. As an example, consider treating a solution of copper(II) sulfate with sodium sulfide solution.  CuSO4(aq) + Na2S(aq)-> CuS(s) + Na2SO4(aq)  What volume of 0.144 M Na2S solution would be required to precipitate all of the copper(II) ion from 27.6 mL of 0.100 M CuSO4 solution?

A 38.5 mL sample of 0.875M AgNO3 solution is mixed with 51.0mL sample of 0.744M NaCl solution. The AgCl precipitated has a mass of 2.06g. Calculate the limiting reactant, the theoretical yield, and the percent yield.AgNO3 (aq) + NaCl (aq) ---> AgCl (s) + NaNO3 (aq)

The concentration of borax (Na₂B4O5(OH)4) in aqueous solution can be determined through titration with HCI as titrant. The net ionic equation for the titration reaction is: B4O5(OH)42 (aq) + 2 H*(aq) + 3 H₂O 4 H3BO3(aq) In an experiment, a student titrated 5.0 mL borax solution with 5.43 0.249 M HCI solution. Determine the concentration of borax in mol/L. For a strong electrolyte compound with formula X3Y2, if the concentration of cation X is 0.614 M, find the concentration of anion Y in mol/L. The molar solubility of a compound AX₂ is 3.8 x 103 M. Calculate the value of natural log of Ksp (Inksp) for AX₂. The enthalpy change (AH) and entropy change (AS) of a process can be obtained by plotting In(Kea) versus 1/Temperature (temperature in Kelvin). A student did the graph and obtained the slope as 7,712 and y-intercept as 6.41, respectively. Determine the enthalpy change of the reaction in kilojoule/mol Question 7 The enthalpy change (AH) and entropy change (AS) of a process can be…

A titration is performed to determine the amount of sulfuric acid, H2SO4,, in a 6.5mL sample taken from a car battery. About 50mL of water is added to the sample, and then it is titrated with 43.37mL of standard 0.5824 molar NaOH solution. How many moles of sulfuric acid are present in the original sample?

What volume in mL of 0.38 M HBr solution is required to titrate 125mL of a 0.18 M Ca(OH)2 solution? Ca(OH)2(aq) + 2HBr(aq) -> CaBr2(aq) + H2O(I)

Consider the neutralization reaction  2HNO3(aq) + Ba(OH)2(aq) yields to 2H2O(L) + Ba(NO3)2(aq) A 0.100 L sample of an unknow HNO3 solution required 49.3 mL of 0.100 M Ba(OH)2 for complete neutralization. What is the concentration of the HNO3 solution?

A sample of a chloride salt weighing 484.6 mg is titrated with AgNO3 using K2CrO4 as indicator. To reach the end point a 52.3 mL of 0.1475 M of AgNO3 solution is required.    The net ionic equation for the reaction of titration is: Ag+ (aq) + Cℓ- (aq) → AgCℓ (s)    How many moles of Ag+ (aq) ions are used to reach the end point?    How many moles of Cℓ- (aq) have reacted in the titration?    How many grams of chloride are present in the sample?   What is the mass percent of chloride in the sample?

By titration, it is found that 62.3 mL of 0.194 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.[HCl]= M