A student mixes 10.00 mL of a 0.00200 M solution of iron(III) nitrate with 2.00 ml. of a 0.00150 M potassium thiocyanate solution and 8.00 mL of water. Before any reaction begins, what are the initial concentrations of iron() ion and thiocyanate ion? Be sure each of your answer entries has the correct number of significant digits. Part 1 of 2 The initial concentration of iron(II)ion= -M Part 2 of 2 The initial concentration of thiocyanate lon ☐M 0.9 X 05 X

imagine that a 2.0 m colution of copper 2 chloride is added to a piece of aluminum.  draw a particulate representation of the mixture after any reaction has completed

A east.cengagenow.com Chemistry I E OWLV2 | Online teaching and learning resource from Cengage Learning According to the following reaction, how m [References) Use the References to access important values if needed for this question. In the laboratory, a student dilutes 15.1 mL of a 10.2 M perchloric acid solution to a total volume of 300.0 mL. What is the concentration of the diluted solution? Concentration = M Submit Answer Try Another Version 10 item attempts remaining Visited es 2 3 a z X C V fn Cengage Learning | Cengage Technical Support DI

A student has 4.20 g of zinc powder, 1.65 L of a 2.40 M calcium nitrate solution, and 1.70 L of a 1.80 M lead(II) nitrate solution.

Suppose that 2.89 L of 6.75 M potassium carbonate is added to 1.38 L of 1.57 M magnesium nitrate.  What is the total concentration of ions in solution after the reaction goes to completion? (Do not include units in your answer. If you round during your calculation make sure to keep at least 3 decimal places. Report your answer to 1 decimal place.)

Please don't provide handwritten solution ....

6. Sodium sulfide reacts with hydrochloric acid to produce hydrogen sulfide and sodium chloride. How many grams of sodium sulfide are required for complete reaction with 15.0 mL of 0.250 M hydrochloric acid? The molar mass of sodium sulfide is 78.046 g/mol. (Hint: start by writing the balanced equation for the reaction.)

You have an unknown solution and you want to determine if it contains ammonia. How will you detect its presence in the laboratory analysis? Please provide two ways to analyze its presence and explain your chosen technique in determining the ammonia.

You wish to make a 0.242 M hydrobromic acid solution from a stock solution of 12.0 M hydrobromic acid. How much concentrated acid must you add to obtain a total volume of 150 mL of the dilute solution?

1) Get two medium test tubes. Into one, place about 2 mL of a solution of copper (II) sulfate. Into the other add about 2 mL of a solution of sodium phosphate. Note the appearence of the two solutions and then mix them together noting any changes that have taken place.  -Changes that take place -Balanced chemical equation -Balanced ionic equation -balanced net ionic equation