A solution contains 0.0490 M Ca²+ and 0.0920 M Ag*. If solid Na3PO4 is added to this mixture, which of the phosphate species would precipitate out of solution first? Ca3(PO4)2 Ag3PO4 O Na3PO4 When the second cation just starts to precipitate, what percentage of the first cation remains in solution? percentage:

When 50.0 mL of a 0.3000 M AgNO3 solution is added to (4.65x10^1) mL of a solution of MgCl₂, an AgCl precipitate forms immediately. The precipitate is then filtered from the solution, dried, and weighed. If the recovered AgCl is found to have a mass of (1.2x10^-1) g. what was the concentration in molarity of chloride ions in the original MgCl₂ solution? 2AgNO3(aq) + MgCl₂(aq) → 2AgCl(s) + Mg(NO3)2(aq) Use the correct number of significant figures and type in the unit abbreviation for the answer. Answer: 8.0x10^-1 M.

Consider the following chemical reaction. 3 Zn(C₂H₃O₂)₂(aq) + 2 Na₃PO₄(aq) → 6 NaC₂H₃O₂(aq) + Zn₃(PO₄)₂(s) A chemist makes a solution of zinc acetate by dissolving 20.5 g Zn(C₂H₃O₂)₂ in 105 mL H₂O. What is the concentration of this zinc acetate solution?

4.) Regarding the fırst preliminary test, what concentration of AGNO3 is required to just cause SO32 ions to precipitate? Assume the concentration of SO32 is 0.10 M. [AGNO3] = _х 107 м

How many grams of Na2SO4 would you need to dissolve in 1.40 L of water in order to create a solution with a concentration of ions equal to 0.725 m? The density of water at this temperature is 0.9881 g/mL

Suppose you are asked to determine the identity of a white solid. When you add water to the white solid, it dissolves and forms a clear solution. When you add a solution of Na, SO,, a white precipitate forms. Add Add H,O Na,SO, Determine the identity of the original solid. O PBCI, O MgCl, O ZNCI, O CaCl,

When 50.0mL of a 0.335M potassium carbonate solution is mixed with 0.045L of a 0.390M nickel(II) chloride solution the following reaction occurs: K2CO3 (aq) + NiCl2 (aq) → a. Complete the reaction equation b. Calculate the mass of precipitate formed c. Calculate the concentration of each ion in the mixture when the reaction is complete

1.58g of magnesium hydrogencarbonate was added to a 1.68 mol/L solution of acetic acid, CH3COOH in water (50.0 mL), producing carbon dioxide gas, water and magnesium acetate, Mg(CH3COO)2. a) Write a balanced chemical equation for the reaction. b) What mass of acetic acid is in the aqueous solution? | c) Which of the reactants is the limiting reagent? Justify your answer. d) If 1.23 g of magnesium acetate was produced, what is the percentage yield of the reaction? e) What is the theoretical yield (in grams) of carbon dioxide from this reaction? f) The above reaction is performed in a closed 25 L container at 10 °C. Upon completion of the reaction, what will the final pressure of CO2 be inside the container?

The spectator ion(s) in the reaction of HCl and NaOH is/are: Na+ OH- OH2O H+ More than one of the above.

If 30.0 g of LiOH is added to 0.650 L of 1.00 M Cd(NO₃)₂, how many grams of precipitate will be formed in the following precipitation reaction?    a) Write a balanced equation. Identify a precipitate. Include states of matter.  b) Determine how much precipitate would form if all reactant 1 ( LiOH) would be used up.  c) Determine how much precipitate would form if all reactant 2 ( Cd(NO3 )2 would be used up.  d) State Limiting reactant , and theoretical yield ( in grams) of the precipitate that would form from the given amounts.