Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (a) Nickel metal is added to a solution of copper(II) nitrate

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (b) a solution of zinc nitrate is added to a solution of magnesium sulfate (c) hydrochloric acid is added to gold metal

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (d) chromium metal is immersed in an aqueous solution of cobalt(II) chloride

Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (e) hydrogen gas is bubbled through a solution of silver nitrate.

The metal cadmium tends to form Cd²⁺ ions. The following observations are made: (i) When a strip of zinc metal is placed in CdCl₂(aq), cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in Ni(NO₃)(aq), nickel metal is deposited on the strip. (a) Write net ionic equations to explain each of the preceding observations.

The metal cadmium tends to form Cd²⁺ ions. The following observations are made: (i) When a strip of zinc metal is placed in CdCl₂(aq), cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in Ni(NO₃)(aq), nickel metal is deposited on the strip. (b) Which elements more closely define the position of cadmium in the activity series?

The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens:

Br₂(aq) + 2 NaI(aq) → 2 NaBr(aq) + I₂(aq)

Cl₂(aq) + 2 NaBr(aq) → 2 NaCl(aq) + Br₂(aq)

(a) Which elemental halogen would you predict is the most stable, upon mixing with other halides?

The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens:

Br₂(aq) + 2 NaI(aq) → 2 NaBr(aq) + I₂(aq)

Cl₂(aq) + 2 NaBr(aq) → 2 NaCl(aq) + Br₂(aq)

(b) Predict whether a reaction will occur when elemental chlorine and potassium iodide are mixed.

(a) Is the number of moles of ions present in a solution an intensive or an extensive property?

(b) Can you identify which one between 0.10 mol ZnCl2 and 0.1M ZnCl2 contains more Zn2+ ion? Why?

You make 1.000 L of an aqueous solution that contains 35.0 g of sucrose (C12H22O11). (b) How many liters of water would you have to add to this solution to reduce the molarity you calculated in part (a) by a factor of two?

(a) Calculate the molarity of a solution that contains 0.175 mol ZnCl₂ in exactly 150 mL of solution.

(c) How many milliliters of a 6.00 M NaOH solution are needed to provide 0.350 mol of NaOH?

a) Calculate the molarity of a solution made by dissolving 12.5 grams of Na₂CrO₄ in enough water to form exactly 750 mL of solution.

(b) How many moles of KBr are present in 150 mL of a 0.112 M solution?

(c) How many milliliters of 6.1 M HCl solution are needed to obtain 0.150 mol of HCl?

A person suffering from hyponatremia has a sodium ion concentration in the blood of 0.118 M and a total blood volume of 4.6 L. What mass of sodium chloride would need to be added to the blood to bring the sodium ion concentration up to 0.138 M, assuming no change in blood volume?

The concentration of alcohol 1CH3CH2OH2 in blood, called the 'blood alcohol concentration' or BAC, is given in units of grams of alcohol per 100 mL of blood. The legal definition of intoxication, in many states of the United States, is that the BAC is 0.08 or higher. What is the concentration of alcohol, in terms of molarity, in blood if the BAC is 0.08?

(a) How many grams of ethanol, CH3CH2OH, should you dissolve in water to make 1.00 L of vodka (which is an aqueous solution that is 6.86 M ethanol)? (b) Using the density of ethanol (0.789 g/mL), calculate the volume of ethanol you need to make 1.00 L of vodka.

(a) Which will have the highest concentration of potassium ions: 0.20 M KCl, 0.15 M K₂CrO₄, or 0.080 M K₃PO₄?

(b) Which will contain the greater number of moles of potassium ion: 30.0 mL of 0.15 M K₂CrO₄ or 25.0 mL of 0.080 M K₃PO₄

Indicate the concentration of each ion or molecule present in the following solutions: (a) 0.35 M K₃PO₄ (b) 1.3×10⁻² M MgSO₄ (c) 0.0184 M CH₃CH₂OH

Ignoring protolysis reactions, indicate the concentration of each ion or molecule present in the following solutions: (d) a mixture of 45.0 mL of 0.272 M NaCl and 65.0 mL of 0.0247 M (NH₄)₂CO₃. Assume that the volumes are additive.

Indicate the concentration of each ion present in the solution formed by mixing: (a) 42.0 mL of 0.170 M NaOH with 37.6 mL of 0.400 M NaOH.

Indicate the concentration of each ion present in the solution formed by mixing: (b) 44.0 mL of 0.100 M Na₂SO₄ with 25.0 mL of 0.150 M KCl

Indicate the concentration of each ion present in the solution formed by mixing: (c) 3.60 g KCl in 75.0 mL of 0.250 M CaCl₂ solution. Assume that the volumes are additive.

(a) You have a stock solution of 14.8 M NH₃. How many milliliters of this solution should you dilute to make 1000.0 mL of 0.250 M NH₃?