HaPO4(aq) + KOH(aq) → KsPOa(ag) + H2O(/) Consider the unbalanced equation above. What is the concentration...
FeCl3(aq) + K2S(aq) → Fe2S3(aq) + KCl(aq) Consider the unbalanced equation above. What is the maximum mass of Fe2S3 that can be produced when 39.0 mL of 0.200 M FeCl3 and 37.0 mL of 0.190 M KZS react?
Given a balanced chemical equation between H2SO4(aq) and KOH(aq) H2SO4(aq) + 2 KOH(aq) → K2SO4(aq) + 2 H2O(l) What volume (in mL) of 0.33 M H2SO4(aq) solution is necessary to completely react with 110 mL of 0.76 M KOH(aq)? Note: (1) The unit of volume of H2SO4(aq) is in mL (2) Insert only the numerical value of your answer (do not include the units or chemical in your answer).
In a solution of Nicly, the cl' concentration is 0.017 M. How many grams of Nicly are in 538 mL of this solution? g NICI the tolerance is +/-2% For the reaction: Na2CO3(aq) + NiCl2(aq) → NICO3(s) + 2NaCl(aq) How many milliliters of 0.38 M NiCl solution are needed to react completely with 31.4 mL of 0.40 M Na2CO3 solution? mL NICI How many grams of Nicoz will be formed? g NICO: What is the molarity of an aqueous solution...
3. Consider the unbalanced reaction shown below: Au+3 (aq) + Ag (s) Ag+1 (aq) + Au (s) A. Write out the balanced equation for this reaction. B. What is Eocell for the spontaneous reaction here? C. Give the expression for Q here that would be used in the Nernst equation. D. What is the value of n to be used in Nernst equation here? E. What would be the value of the slope if Ecell were plotted vs log Q...
Review equation 16.10 and step B2. Ag+1(aq) and NH3(aq) will form a soluble complex ion. Use rule 3 of Water-Insoluble Salts in Appendix E to determine what would happen if Ag+1(aq) was combined with KOH instead of NH3. Write the net ionic equation with phase subscripts, where K+1 is a spectator ion which is cancelled out. Equation 16.10: Ag^+(aq) + Cl^-(aq) ⇄ AgCl(s) ⇅ 2NH3(aq) [Ag(NH3)2]^+(aq) Step B2: Silver Chloride equilibrium. To the clear solution from part B.1, add 5...
Consider the unbalanced redox reaction: MnO−4(aq)+Zn(s)→Mn2+(aq)+Zn2+(aq) Balance the equation in acidic solution. Part B- Determine the volume of a 0.475 M KMnO4 solution required to completely react with 3.35 g of Zn.
Consider the unbalanced redox reaction: Cr2O2−7(aq)+Cu(s)→Cr3+(aq)+Cu2+(aq) Part A Balance the equation. Part B: Determine the volume of a 0.750 M K2Cr2O7 solution required to completely react with 4.25 g of Cu.
Consider the unbalanced redox reaction occurring in acidic solution: MnO−4(aq)+Zn(s)→Mn2+(aq)+Zn2+(aq) Part A Balance the equation in acidic solution. Express your answer as a chemical equation. Identify all of the phases in your answer. Part B Determine the volume of a 0.200 M KMnO4 solution required to completely react with 2.40 g of Zn. Express your answer using three significant figures.
16. What is the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine to form lithium nitride, a component of advanced batteries, according to the following unbalanced equation? Li+N, — LizN 17. What is the concentration of NaCl in a solution if titration of 15.00 mL of the solution with 0.2503 M AgNO, requires 20.22 mL of the AgNO3 solution to reach the end point? AgNO3(aq) + NaCl(aq) AgCl(s) +NaNO (aq) 18. In a common medical...
Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride: Ag+(aq)+Cl−(aq)→AgCl(s) Silver chloride is virtually insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0 mL of 0.149 M AgNO3 solution to completely precipitate the silver?