The balanced chemical equation for the reaction is-
KOH + NiSO4 = K2SO4 + Ni(OH)2
This is double displacement reaction in which two reacting ionic compounds (here, KOH and NiSO4) exchange their corresponding ions
( i.e. K+ ,OH-,Ni2+,SO42- ).
A solution of 100.0 mL of 0.200 M KOH is mixed with solution of 200.0 mL...
A solution of 116 mL of 0.160 M KOH is mixed with a solution of 230 mL of 0.180 M NiSO4. Write the balanced chemical equation for the reaction that occurs. Express your answer as a balanced chemical equation. Identify all of the phases in your answer.
When 1.50 mL of 3.5-M Barium chloride is mixed with 2.50 mL of 0.65-M sodium sulfate, a precipitate forms. a. Write balanced chemical, ionic and net ionic equations for the reaction, including phase labels. b. Calculate the theoretical yield (in grams) of the precipitate and identify the limiting reactant. c.Calculate the grams of the reactant in excess (left over) after the reaction is complete.
A 829.0-mL aliquot of 0.880 M aqueous potassium hydroxide is mixed with 829.0 mL of 0.880 M aqueous magnesium nitrate. ( just need d.) a.)Write a balanced chemical equation for any reaction that occurs. b.) The precipitate is magnesium hydroxide Mg(OH)2 c.) What mass of precipitate is produced? d.)Calculate the concentration of each ion remaining in solution after precipitation is complete. Assume that the precipitate is completely insoluble The concentration of K+ = ____ M The concentration of OH- =...
375 mL of a 0.150 M aqueous solution of silver (I) nitrate is mixed with 125 mL of a 0.125 M aqueous solution of sodium phosphate. Calculate the mass of precipitate that forms and the final concentration of each ion in the mixed solution. Volumes are additive and the precipitation reaction goes to completion. Can you show all work for calculating the final concentration of each ion in the reaction including Ag, NO3^-1, Na and PO4^-3
200.0 mL of a solution of 2.000M MgCl2 was mixed with equal amount of 2.000M Na2CO3and MgCO3 precipitate was collected (MgCO3 Ksp = 1.580x10?8). How much (how many grams) of the precipitate was collected? What is the final concentration of the [Mg] in the solution? Steps would be appreciated!
18. A 200.0-mL sample of a 0.0015 M copper(II) nitrate solution is mixed with a 250.0-mL sample of 0.20 M NH3. After the solution reaches equilibrium, what concentration of copper(II) ion remains? You will have to look up the appropriate complex formation constant.
7. In the lab one day, you mixed 30.0 mL of a 0.500 M Na:CO) solution with 45.0 mL of a 0.667 M Cr(N0)) solution. Write a balanced chemical equation complete with physical states: a. Write the ionic equation for the reaction: b. ENG 2 C- CraCoo) c. Write the net-ionic equation for the reaction: 2 C Calculate the mass of the precipitate formed (hint: find the limiting reactant) d. Calculate the molarities of ions remaining in solution after the...
If I mixed 100.0 mL of a nitric acid solution of pH = 2.40 with 100.0 mL of a nitric acid solution of pH = 2.70, what would be the pH of the mixture? Write your answer to 2 digits beyond the decimal (e.g., 8.63) If 5.15 grams of iron(III) nitrate (molar mass = 241.86 g/mol) is dissolved in enough water to prepare exactly 150.0 mL of solution, what would be the molar concentration of the nitrate ion? 0.284 M...
When 200.0 ml of 0.270 M Mgcl2 solution reacts with with 300.0 ml of 0.160 M K3Po4 solution a precipitate forms. A) Determine the molarity of the chloride ion after the reaction has occured.
Write the balanced neutralization reaction that occurs between H2SO4 and KOH in aqueous solution. Phases are optional. neutralization reaction: Suppose 0.350 L of 0.490 M H2SO4 is mixed with 0.300 L of 0.200 M KOH . What concentration of sulfuric acid remains after neutralization?