Potassium iodide reacts with lead(II) nitrate in the following precipitation reaction:2 KI(aq) + Pb(NO3)2(aq)¡2 KNO3(aq) + PbI2(s)What minimum volume of 0.200 M potassium iodide solution is required to completely precipitate all of the lead in 155.0 mL of a 0.112 M lead(II) nitrate solution?a) 348 mL b) 86.8 mLc) 174 mL d) 43.4 mL

If 2.00 grams of an unknown DIPROTIC acid (H2A) is titrated with 34.0 mL of 1.35 M NaOH, what is the molar mass (g/mol) of the diprotic acid? H2A+2NaOH⟶2H2O+Na2AH2A+2NaOH⟶2H2O+Na2A (Hint: See equation below in which mm is molar mass (units: g/mol), m is mass (unit: g), and mol isnumber of moles (unit: mol)). mmacid=macidmolacidmmacid=macidmolacid Molar Mass =  ___________   g/mol (input the numeric value only!) Remember: use correct significant figure rules. Significant figures always matter in Chemistry!

Fe(lI) can be precipitated from a slightly basic aqueous solution by bubbling oxygen through the solution, which converts Fe(ll) to insoluble Fe(lI): 4Fe(OH)*(aq) +40H¯(aq)+O2(g) +2H,0(1) → 4Fe(OH),(s) How many grams of O2 are consumed to precipitate all of the iron in 50.0 mL of 0.0950 MFe(II)?

A 10.00 mL vinegar sample is pipetted into an Erlenmeyer flask and titrated with 24.77 mL of 0.575 M NaOH to a permanent endpoint. Calculate the molarity of the acetic acid (HC2H3O2 60.06 g/mol) in the vinegar.

50.0 mL of a 0.4230 M solution of Na3PO, was mixed with 100.0 mL of 0.5151 M HgNO3 and allowed to react: Na3PO4 (aq) + HgNO3(aq) → 3 NaNO3(aq) + Hg3PO4 (s) - Answer the following questions: What mass of precipitate was formed? What is the molarity of the unreacted reactant after the reaction is complete? Check 9 M

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…

1-A 15.0 mL solution of Sr(OH)₂ is neutralized with 35.6 mL of 0.350 M HCl. What is the concentration of the original Sr(OH)₂ solution? 2-If 15.5 g of NaOH is added to 0.550 L of 1.00 M Ni(NO₃)₂, how many grams of Ni(OH)₂ will be formed in the following precipitation reaction? 2 NaOH(aq) + Ni(NO₃)₂(aq) → Ni(OH)₂ (s) + 2 NaNO₃ (aq) 3-You add 475 mL of water to 40.0 mL of 0.550 M MgCl₂ solution. Assuming the volumes are additive, what is the MgCl₂ concentration in the diluted solution?

10) A beaker contains 0.300 L of a 0.20 M Pb(NO3)2 solution. If 0.200 L of a 0.20 M solution of MgCl2 is added to the beaker, what will be the final excess moles of Pb^+2 ions in the resulting solution?

A student is titrating a vinegar solution to determine the acetic acid (HC2H3O2) content. They add exactly 10.00 mL of the solution to a flask with a few drops of phenolphtahalein, and titrate it with an NaOH solution. The NaOH concentration is 0.6 M and it takes 12.04 mL to neutralize the acid and reach the endpoint. What is the molar concentration (M) of the acetic acid in the vinegar solution?

Suppose you are titrating a solid mixture containing  KHPKHP  (molar mass=204.2 g/mol) and a salt compound.  KHPKHP  reacts with  NaOHNaOH  according to the equation     KHP+NaOH⟶H2O+NaKPKHP+NaOH⟶HX2O+NaKP   You prepare the analyte from 0.507 g of the  KHPKHP  mixture. You then require 11.35 mL of 0.101 M  NaOHNaOH  solution to complete the titration.   What is the percentage of  KHPKHP  in the mixture?