Calculate the concentration (M) when 54.3 g of NaOH (40.0 g/mol) are used to prepare 2886.0 mL of solution.
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Calculate the concentration (M) when 54.3 g of NaOH (40.0 g/mol) are used to prepare 2886.0...
How many grams NaOH (40.0 g/mol) are required to make 250 mL of a 0.500 M solution?
6. a) Calculate the volume in litres for 5.00 mol NaOH from a 12.0 M NaOH solution. b) Calculate the volume in litres for 15.0 g of Na2SO4 from a 4.00 M Na2SO4 solution. c) Calculate the mass of solute required to prepare 25.0 mL of a 5.0 M HCl solution.
25.0 mL of 0.100 M NiSO4 solution is added to 50.0-mL of a 0.080 M NaOH solution. NiSO4(aq) + 2 NaOH(aq) -> Ni(OH)2(s) + Na2SO4(aq) a. What is the limiting reagent? b. What is the mass of precipitate formed? c. After the reaction is complete, calculate the concentration of the reactant remaining in solution. ( NiSO4 = 158.8 g/mol | NaOH = 40.0 g/mol | Ni(OH)2 = 92.7 g/mol )
40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH. After 20.0 mL of the base solution has been added, the pH in the titration flask is 5.10. What was the concentration of the original acetic acid solution? [Ka(CH3COOH) = 1.8 × 10–5]
Calculate the final concentration of the solution when water is added to prepare each of the following solutions. 22.0 mL of a 10.0 %(m/v) K2SO4 solution is diluted to 60.0 mL & 80.0 mL of a 7.60 M NaOH solution is diluted to 245 mL
3) A solution is prepared by adding 40.0 mL of 0.060 M NaOH and 40.0 mL of 0050 M Sr(OH) a) Calculate the concentrations ofall ions in solution. b) Calculate the pOH of this solution.
5.) A solution is prepared by adding 40.0 mL of 0.060 M NaOH and 40.0 mL of 0.050 M Ca(OH)2 (a) Calculate the concentrations of all ions in solution. (b) Calculate the pOH of this solution.
Calculate the concentration of a NaOH solution whose equivalence point was determined to be when 24.40 mL of 0.125 mol L^-1 HCI was added to the initial 25.0mL sample of NaOH solution. Molarity = amount of (mol) /volume (litres) Concentration /mol L^-1 = _________ please give me the answer thank you :)
A 40.0 mL solution containing 0.500 g of KHP was titrated with NaOH solution of unknown concentration, and the pH of the solution was measured after each known amount of NaOH was added. (KHP=potassium hydrogen phthalate; formula=KHC8H4O4; molar mass=204.22 g/mol). The acid base reaction occurs according to the following net ionic equation: HC8H4O4- (aq) + OH- (aq) ®C8H4O42- (aq) + H2O What is the molar concentration of KHP in the solution? If the titration required 24.0 mL of NaOH to...
A solution of NaOH has an unknown concentration. When 1.396 g of potassium hydrogen phthalate (KHP a monoprotic acid frequently used as an analytical standard) is titrated with the sodium hydroxide the end point is 42.54 mL. Use this information to compute the concentration of NaOH in the solution. The molar mass of KHP is 204.22 g mol1. [OH mol L