The reaction between hydrochloric acid and sodium carbonate is represented by the equation 2HCI(ag) + Na2CO3(ag) → 2NAC((ag) + H20(1) + CO2(g) If 25.0 mL of 0.050 M sodium carbonate solution is neutralised by 50.0 mL of hydrochloric acid, the concentration of the hydrochloric acid must be ... M 0.01 O M 0.025 O M 0.05 O M 0.10 O

The molarity of an aqueous solution of potassium hydroxide,KOH, is determined by titration against a 0.234M nitric acid,HNO3,solution.   If 29.6 mL of the base are required to neutralize 21.9 mL of nitric acid, what is the molarity of the potassium hydroxidesolution? Molarity = M

Consider the reaction: Ag⁺(aq) + Cl⁻(aq) → AgCl(s) How many grams of NaCl would be needed to precipitate the Ag⁺ ions from 2.650 × 10² mL of a 0.0115 M AgNO₃ solution? The molar mass of NaCl is 58.44 g/mol.

A student needs to dilute a 0.47 M Pb(NO3)2  solution to make 77.0 mL of 0.22 M Pb(NO3)2. Set up the calculation by placing the values with the correct units into the equation. Then, calculate the volume, in milliliters, of the 0.47 M Pb(NO3)2 solution that is needed.

Consider the reaction: Ag⁺(aq) + Cl⁻(aq) → AgCl(s) How many grams of NaCl would be needed to precipitate the Ag⁺ ions from 2.600 × 10² mL of a 0.0115 M AgNO₃ solution? The molar mass of NaCl is 58.44 g/mol.

A 2.00 g sample of KCl is dissolved in 60.0 mL of water. The resulting solution is then added to 20.0 mL of a 0.830 M CaCl2 (aq) solution. Assuming that the volumes are additive, calculate the concentrations of each ion present in the final solution. Concentration of K+ ions = M Concentration of Ca 2+ ions = M Concentration of Cl¯ ions = M

A sample of solid Mg(OH)2 was stirred in water at a certain temperature until the solution contained as much dissolved Mg(OH)2 as it could hold. A 450-mL sample of this solution was withdrawn and titrated with 0.00357 M HClO4. It required 58.3 mL of the acid solution for neutralization.What is the solubility of Mg(OH)2 in water, at the experimental temperature, in grams of Mg(OH)2 per liter of solution?

A 10.00 ml sample of a solution of acetic acid in water was titrated to the endpoint by the addition of 15.89 ml of 0.2432 M NaOH. Calculate the volume of this NaOH solution that would be required to titrate 50.00 ml of vinegar. Vinegar is 5.00% (by mass) acetic acid. Assume that the density of the vinegar solution is the same as that of water (1.00 g/ml).

Jake carried out three titrations to determine the concentration of unknown nitric acid (HNO3) using 0.1050 M NaOH. He titrated 100.0 mL of the nitric acid sample and obtained the following volumes of NaOH: 20.56, 20.48, and 20.52 mL. The acid-base reaction occurring is NaOH (aq) + HNO3(aq) →→ NaNO3(aq) + H2O(l) Determine the concentration of the acid; report the average molarity with standard deviation. Pay attention to the number of significant figures on the mean and the number of decimal places on the standard deviation.

The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated as KHP). KHP is an acid with one acidic hydrogen and a molar mass of 204.22 g/mol. In the titration, 48.82 mL of the sodium hydroxide solution was required to react with 0.7540 g KHP. Calculate the molarity of the sodium hydroxide. Molarity = ___________ M