Calculate the number of milliliters of 0.762 M NaOH required to precipitate all of the Pb²+ ions in 173 mL of 0.797 M Pb(NO3)2 solution as Pb(OH)2. The equation for the reaction is: Pb(NO3)2(aq) + 2NAOH(aq) Pb(OH)2(s) + 2NANO3(aq) mL NAOH

Calculate the number of milliliters of 0.580 M Ba(OH)2 required to precipitate all of the Cu2+ ions in 120 mL of 0.745 M CuCl2 solution as Cu(OH)2. The equation for the reaction is:CuCl2(aq) + Ba(OH)2(aq) Cu(OH)2(s) + BaCl2(aq) mL Ba(OH)2

The following chemical reaction takes place in aqueous solution: 2 AgNO3(aq) + (NH4), CO3(aq) →Ag₂CO3(s)+2 NH¸NO₂(aq) Write the net ionic equation for this reaction. 0

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 15.0 mL of 0.500 M Ba(OH)2 is required to titrate a 10.0 mL of an unknown solution of HNO3, according to the following equation:       Ba(OH)2(aq) + 2HNO3(aq) → Ba(NO3)2(aq + 2H2O(l).  What is the concentration of the HNO3 solution?

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)

A 25.00 mL sample of boric acid requires 32.57 mL of 0.2514 M NaOH to reach the endpoint of titration. H3BO3 (aq) + 3 NaOH (aq) → Na3BO3 (aq)   + 3 H2O (l) Determine the concentration of boric acid in the sample. Write the full and net ionic equation for the reaction.

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?

A student titrates 22.00 mL of an unknown HCI solution with 27.00 mL of a 0.5090 M Ca(OH)2 solution. What is the molarity of the unknown acid?

A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 86. mg of oxalic acid (H,C,04), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 37.0 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits. x10