You have 75.0 mL of a 2.50 M solution of Na2CrO4(aq). You also have 125 mL of a 2.01 M solution of AgNO3(aq). Calculate the concentration of CRO42-after the two solutions are mixed together.

A 0.450 g sample of impure CaCO,(s) is dissolved in 50.0 mL of 0.150 M HC1(aq). The equation for the reaction is CACO, (s) + 2 HCI(aq) → CaCl, (aq) + H,O(1) + CO,(g) The excess HCl(aq) is titrated by 8.60 mL of 0.125 M NAOH(aq). Calculate the mass percentage of CaCO, (s) in the sample. mass percentage: % Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry Publisher: University Science Books O O 6 hulu 9 MacBook PrO GSearch or type URL % & 4. 6. 8. dele Y. OP H. V MOSISO command option

Mg(s) + 2H2O(l) = Mg(OH)2(aq) + H2(g) What is the concentration of hydroxide ions in the solution formed when 4.00g of Mg(s) react with sufficient water to form 200. mL of solution?

The amount of nitrogen in an organic substance can be determined by an analytical method called the Kjeldahl method, in which all the nitrogen in the organic substance is converted to ammonia. The ammonia, which is a weak base, can be neutralized with hydrochloric acid, as described by the equation NH3(aq) + HCl(aq) ->> NH₂Cl(aq) If 6.0 mL of 0.150 M HCl(aq) is needed to neutralize all the NH3(g) from a 2.25 g sample of organic material, calculate the mass percentage of nitrogen in the sample.

To a 25.00 mL volumetric flask, a lab technician adds a 0.100 g sample of a weak monoprotic acid, HA, and dilutes to the mark with distilled water. The technician then titrates this weak acid solution with 0.0841 M KOH. She reaches the endpoint after adding 44.65 mL of the KOH solution. Determine the number of moles of the weak acid in the solution. moles of weak acid: Determine the molar mass of the weak acid. molar mass= pKa mol After the technician adds 16.63 mL of the KOH solution, the pH of the mixture is 5.79. Determine the pK₁ of the weak acid. = g/mol

You have been provided with a 2.08 x 10-2 L  sample of lithium hydroxide (LiOH) of unknown concentration. You perform a titration with 2.19 M nitric acid (HNO3), and find that 24.6 mL are required to reach the equivalence point (as determined using a coloured indicator). What is the concentration of the lithium hydroxide solution in mol L-1?

Titration is a common laboratory method of quantitative chemical analysis. In an acid- base titration, 65.0 mL of Ba(OH)2 was neutralized by 58.0 mL of 0.350 mol/L HCl. Calculate the concentration of Ba(OH)

A titration is a procedure for determining the concentration of a solution by allowing it to react with another solution of known concentration (called a standard solution). Acid-base reactions and oxidation- reduction reactions are used in titrations. For example, to find the concentration of an HCl solution (an acid), a standard solution of NaOH (a base) is added to a measured volume of HCI from a calibrated tube called a buret. An indicator is also present and it will change color when all the acid has reacted. Using the concentration of the standard solution and the volume dispensed, we can calculate molarity of the HCl solution. A volume of 90.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H₂SO4). What was the molarity of the KOH solution if 13.2 mL of 1.50 M H₂SO4 was needed? The equation is 2KOH(aq) + H₂SO4 (aq)→K₂SO4 (aq) + 2H₂O(1) Express your answer with the appropriate units. ► View Available Hint(s) molarity = Submit…

By titration, it is found that 55.5 mL of 0.116 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution. [HCI] M

By titration it is found that 35.7 mL of 0.101 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.