A chemistry student in the laboratory titrated 18.00 mL of HCl solution with 58.6 mL of 0.145 M NaOH solution to the endpoint. (See chemical reaction for the titration below.) HCl (aq) + NaOH (aq) --> NaCl (aq) + H2O (aq) What is the unknown molarity of the HCl solution?

A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 30. mg of oxalic acid (H,C,0,), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 62.3 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits. x10

A student prepares a dilute solution of sodium hydroxide, NaOH (aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point.   A.) If the titration required 21.84 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate, KHC8H4O4, NOT potassium hydrogen phosphorus!)   B.) The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phenolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar.   C.) Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the molar concentration for acetic acid, HC2H3O2 (aq), determined in part b and assuming the density of the solution is 1.01 g/mL.

A chemistry student weighs out 0.159 g of ascorbic acid (H,C,H,0), a diprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.0800M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits. mL

You have a 1.153 g sample of an unknown solid acid, HA, dissolved in enough water to make 20.00 mL of solution. HA reacts with KOH(aq) according to the following balanced chemical equation:HA(aq)+KOH(aq) --------->KA(aq)+H2O(l)       If 14.90 mL of 0.585 M KOH is required to titrate the unknown acid to the equivalence point, what is the concentration of the unknown acid? ______ M      What is the molar mass of HA? _____  g/mol

What volume (in mL) of  0.50 M NaOH is required to completely titrate 25.0 mL of 1.2 M H2SO4? 2 NaOH(aq)  +  H2SO4(aq) → Na2SO4(aq) + 2 H2O(l)

You are performing an experiment in lab that involves the titration of a H2SO4 solution. You titrate the acidic solution with 0.5166 M NaOH and the equivalence point is reached by the addition of 21.76 mL of NaOH solution. Using the balanced equation below, calculate the moles of H2SO4 in the flask. Do NOT include units or write the answer in scientific notation. 2NaOH(aq) + H2SO4(aq) → 2H2O(l) + Na2SO4(aq)

Write a balanced net-ionic equation for the neutralization reaction between CH3COOH (aq) and Ba(OH)2 (aq). 2 CH3COOH (aq) + Ba(OH)2 (aq) --> 2 CH3COO- (aq) + 2 H₂O (1) + Ba²+ (aq) 2 CH3COOH (aq) + 2 OH" (aq) --> 2 CH3COO(aq) + 2 H₂O (1) CH3COOH (aq) + OH" (aq) --> CH3COO (aq) + H₂0 (1) OH(aq) + OH- (aq) --> H₂O (1) 2 H (aq) + 2 OH- (aq) --> 2 H₂O (1)

If 50.0 ml of 1.00 M MgCl2 is added to 50.0 ml of 1.00M NaOH, solid Mg(OH)2 forms according to the following equation     MgCl2 (aq)   +  2 NaOH(aq)  -->   Mg(OH)2( s)   +  2 NaCl (aq)  (95.20g/mol)        (40.00g/mol)   (58.32 g/mol)    (58.44 g/mol) What is the limiting reactant in this reaction?

A chemistry student weighs out 0.0856 g of citric acid (H,CH,0,), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.0900 M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits. mL x10