Write the balanced chemical equation based on the following description: aqueous calcium hydroxide reacts with aqueous nitric acid to produce the aqueous calcium nitrate and liquid water.

now you return to the test tube containing Group III ions. After testing, you have a pink precipitate. Explain the identity of the Group III ions and how you came to this conclusion

Suppose 0.274 g of lead(II) acetate is dissolved in 100. mL of a 23.0 mM aqueous solution of ammonium sulfate. Calculate the final molarity of acetate anion in the solution. You can assume the volume of the solution doesn't change when the lead(II) acetate is dissolved in it.

A student adds 10.2 mL of 7.06 M of nitric acid to 0.5502 g copper turnings. What volume of 3.44 M sodium hydroxide would be required to neutralize the acid, assuming that none of the nitric acid was consumed in the previous step of the experiment?

Enter your answer in the box provided. A 2250 mL sample of 2.50 M HCl solution is treated with 4.14 g of magnesium. Calculate the concentration of the acid solution after all the metal has reacted. Assume that the volume remains unchanged. M HCI ences

How many grams of solid calcium hydroxide are needed to exactly neutralize 17.4 mL of a 1.30 M nitric acid solution ? Assume that the volume remains constant

What is the sulfide ion concentration in a solution prepared by mixing together a 340.0 mL, 0.18 M sodium sulfide solution and a 188 mL, 0.18 M, iron (III) perchlorate solution? Don't forget to take into account that iron (III) sulfide will precipitate from solution as a solid.

The zinc content of a 1.07 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc. The excess HC1 is then neutralized with with NaOH. The reaction of HC1 with Zn is shown. Zn(s) + 2 HCl(aq) → ZnCl₂ (aq) + H₂(g) The ore was dissolved in 150 mL of 0.600 M HCl, and the resulting solution was diluted to a total volume of 300 mL. A 20.0 mL aliquot of the final solution required 9.96 mL of 0.540 M NaOH to neutralize the excess HC1. What is the mass percentage (%w/w) of Zn in the ore sample? %W/W = % Zn

N21.

2. 2.00G of aluminum solid is added to a 100.0 mL of 2.5 M aqueous solution of hydrobromic acid. 2a. write the net ionic equation