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

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 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 16.8 mL of HNO₃ was required. Write the balanced chemical equation based on the following description: solid calcium hydroxide reacts with aqueous nitric acid to produce the aqueous calcium nitrate and liquid water.  Ca(OH)2(aq)+HNO3(aq)------

If 28.0 g of NaOH is added to 0.600 L of 1.00 M Mn(NO₃)₂, how many grams of Mn(OH)₂ will be formed in the following precipitation reaction? 2 NaOH(aq) + Mn(NO₃)₂(aq) → Mn(OH)₂ (s) + 2 NaNO₃(aq)