A solution was prepared in the lab when equal volumes of 3.00 x 10-4 M calcium chloride and 1.00 × 10-4 M lithium phosphate were combined. Will a precipitate form? A solution was prepared in the lab when equal volumes of calcium chloride and lithium phosphate were combined. Write the formula for the calcium phosphate salt.

A solution contains Cr3+ and Mg2+. The addition of 1.00 L of 1.51 M NaF solution is required to cause the complete precipitation of these ions as CrF3(s) and MgF2(s). The total mass of the precipitate is 50.1 g . Find the mass of Cr3+ in the original solution.

A 24.8mL sample of vegetable juice is titrated with 15.65mL of NaOH solution. The molar concentration of the NaOH is .106 M. The molar mass of citric acid is 192.12 g-mol-1. Express all with three significant figures.  A) Determine the molar concentration of citric acid in the vegetable juice sample B) Determine the number of moles of citric acid per 240 mL of the vegetable juice.  C) Determine the mass of citric acid per 240 mL of the vegetable juice.  D) If the label on the bottle lists the citric acid contest as 1g per serving with a serving size of 240 mL determine the percent error in the rotation results. Express in 2 sig figs.

What is the precipitate formed upon mixing mercurous nitrate and sodium chloride? O Hg:Cl: Hg:(NO.): NANO: O none of these What is the precipitate formed upon mixing silver nitrate and calcium chromate? O Ca(NO:)2 CaCro. Ag:CrO. O none

12. In a titration of HNO3, you add a few drops of phenolphthalein indicator to 50.00 L if acid in a flask. You quickly add 20.00 mL of 0.0502 M NaOH but overshoot the endpoint, turning the solution a deep pink color. Instead of starting over you add an additional 30.00 mL of the acid, turning the solution colorless. It then takes 3.22 mL of the NaOH to reach the endpoint. a. Write the Molecular, Total Ionic, and Net Ionic Equations for this reaction. b. What is the concentration of the HNO3 solution? c. How many moles of NaOH were in excess after the first addition?

Solid potassium hydroxide is slowly added to 75.0 mL of a chromium(III) nitrate solution until the concentration of hydroxide ion is 0.0417 M. The maximum amount of chromium(III) ion remaining in solution is M.

The four solutions were made and then mixed in the following order. 1. Starting with 0.100M Bacl2 100.0 mL 2. Adding 0.100M AgNo3 50.0 mL 3. Adding 0.100M H2SO4 50.0 mL 4. Added 0.100M NH3 250.0 mL Write a response formula for the response that takes place after each step, assume that all the responses are complete and calculate the concentration of Ba2+, Cl-, NH3 and NH4+ in the final solution.

1.     Reaction Add 1 drops of … Add 1 drops of… Did a precipitate form?   1 Fe(NO3)3         Na3PO4   2 AgNO3   3 Zn(NO3)2   4 Al(NO3)3   5 Pb(NO3)2

A 30.00 ml sample of sulfuric acid is titrated to the endpoint with a 0.1000 M potassium hydroxide solution. The initial buret reading was 3.04 mL; the final reading was 45.52 mL. What is the molarity of the acid solution?     0.0759     0.0472     0.0708     0.283     0.0353