Determine the molar concentrations of Ca2+ and Cl- in a 0.38 M calcium chloride?

An aqueous solution of calcium chloride is labeled 0.010 M CaCl2. What is the molar concentration of CaCl2, Ca+, and Cl- in the aqueous solution? Explain.

Calculate the concentration in molarity of Fe3+ in 0.69 M Fe2(SO4)3 . (Answer format x.xx - 2 decimal places - no units)

Determine the concentrations of Na2CO3, Na+, and CO32− in a solution prepared by dissolving 2.20 × 10−4 g Na2CO3 in 1.00 L of water. Express all three concentrations in molarity. Additionally, express the concentrations of the ionic species in parts per million (ppm). Note: Determine the formal concentration of CO32−. Ignore any reactions with water. Thanks!

Moly Cule is also mixing a solution of calcium fluoride (CaF2). If she adds some Aqueous Calcium Oxide (CaO) to the solution, can she eventually get some solid CaF2 to form? What dictates how much Ca2+ and F- are in solution, and how much are in solid CaF2. Since Ca(OH)2 is a strong base and HF is a weak acid, would adding some strong NaOH (another strong base) to the solution cause a precipitate to form? Why or why not?

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 10.0 mL sample of 0.20 mol/L NiF2(aq) is mixed with 20.0 mL of 0.0700 mol/L NaOH(aq) and then diluted to a final volume of 100. mL. Calculate the concentration of OH- ions in the 100 mL mixture before the reaction starts. Express your answer to three significant figures.

6. A buffer is prepared by adding 20.0 g of sodium acetate (CH3COONa) to 500 mL of a 0.150 M acetic acid (CH3COOH) solution. (A) write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the buffer. (B) Write the complete ionic equation for the reaction that occurs when few drops of sodium hydroxide solution are added to the buffer. Group of answer choices a.) (A) CH3COO-(aq)+ H+ (aq) --->CH3COOH(aq) (B) CH3COOH(aq) + OH-(aq)--->CH3COO-(aq)+H2O(l) b.) (A) Na+ (aq)+ CH3COO-(aq)+ H+ (aq)+CI-(aq) --->CH3COOH(aq)+Na+(aq)+CI-(aq) (B) CH3COOH(aq)+Na+(aq)+ OH-(aq)--->CH3COO-(aq)+H2O(l)+Na+(aq) c.) (A) Na+ (aq)+ CH3COO-(aq)+ H+ (aq)+CI-(aq) --->CH3COOH(aq)+Na+(aq)+CI-(aq) (B) CH3COOH(aq) + OH-(aq)--->CH3COO-(aq)+H2O(l) d.) (A) CH3COO-(aq)+ H+ (aq)  --->CH3COOH(aq) (B) CH3COOH(aq)+Na+(aq)+ OH-(aq)--->CH3COO-(aq)+H2O(l)+Na+(aq)

A sodium hydroxide solution is standardized by titrating 0.8592 g of ordinary standard potassium hydrogen phthalate (204.22 g/mol) to a phenolphthalein end point, requiring 32.67 ml. What is the molarity of the NaOH solution? cO,K cO;K + NaOH + H,0 COH Pim yg pla

Using the square-bracket notation, express the concentration of chloride ions in a solution that is 0.250 M in sodium chloride(NaCl) and 0.25 M in magnesium chloride (MgCl2).