If it required 23.9 mL of 0.0150 M Ca(OH)2 to neutralize 25.0 mL of HNO3 , what was the initial concentration of the nitric acid solution?

A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 20.2 mL of HNO₃ was required. How many moles of Ca(OH)2 had to be present in the initial reaction?

What is the concentration of nitrate ions in a 0.200 M Ca(NO3)2 solution?

A 50.00 mL sample of a locally made white wine required 34.50 mL of 0.0450 M NaOH to reach the end point. Express the acidity of the wine in grams of tartaric acid (H­2C4H4O6)

How many mL of 0.022 M HCl would it take to completely neutralize 14.11 mL of 1.16 M Ca(OH)2 according to the following reaction equation. 2HCl + Ca(OH)2 --> 2H2O + CaCl2

What is the concentration of F— ions when 266.640 mg of MgF2 (62.3018 g/mol) completely dissociates in 2.442 L of water?

A 50.0 mL solution of Ca(OH)2 with an unknown concentration was titrated with 0.340 M HNO3. To reach the endpoint, a total of 28.4 mL of HNO3 was required. Given that 0.00966 mol of HNO3 are used in the titration, What quantity in moles of Ca(OH)2 had to be present in the initial reaction? mol 1 3. 4 C 7 8. +/- х 10 LO

Determine the molarity of NaOH to three decimal places if 20.19 mL of this NaOH were used to titrate 0.323 g of KHP (MM 204.22 g/mol)

How many grams of solid BaSO4 will form when excess 0.25M Na2SO4 reacts with 25 mL of 0.50 M Ba(NO3)2?

A student is preparing 250 mL of a solution of 155.0 mM NaCl in 50.0 mM phosphate pH 6.4.  The student has stock solutions of 0.850 M NaCl and 0.400 M phosphate pH 6.4.  Calculate the volume of phosphate required to make the solution (in mL).