You have 825.0 mL of 0.550 M aqueous NaCl. For each of the following statements, determine...

You have 825.0 mL of 0.550 M aqueous NaCl. For each of the following statements, determine whether the statement is true of false.

If the statement is true, type "true" in the blank next to the statement.

If the statement is false, type "false" in the blank next to the statement.

________ There are 825 mL of solution

________ If you add water to the solution, the molarity will increase.

________ There is 0.550 moles of NaCl in 825 mL of solution.

________ NaCl is the solvent.

Expert Solution

Given 825 ml of 0.55 M aq NaCl solution is present which means that no of moles of NaCl =(0.825*0.55)=.45375 moles is present in 825 ml of solution .(Note: Molarity=no of moles of solute/Volume of solution(in litres))

so It is true that 825 ml of solution is present.

Molarity is defined as number of moles of solute present in a litre of solution so if you add water then volume of solution increases and hence molarit will decrease. So 2nd statement is false.

As calculated above no of moles of NaCl=0.45375 moles so 3rd statement is false.

NaCl is the solute as it is present in small amount while water is solvent here as phase is aqueous in nature.So this statement is false

queen_honey_blossom answered 2 years ago

Calculate the molality of each of the following aqueous solutions: (a) 2.01 M NaCl (density of...

Calculate the molality of each of the following aqueous solutions: (a) 2.01 M NaCl (density of solution = 1.08 g/mL) m (b) 51.8 percent by mass KBr solution

You have 100. mL of aqueous 0.40 M CuSO4 mixed with 100. mL of aqueous 0.20...

You have 100. mL of aqueous 0.40 M CuSO4 mixed with 100. mL of aqueous 0.20 M Na2S. 1. What kind of reaction could potentially take place? (a) Bronsted-Lowry acid base (b) redox (c) precipitation (d) no reaction 2. Which of the following is/are the spectator ions in this reaction? (a) SO42- (b) Na+ (c) S2- (d) Cu2+ 3. After the solutions are mixed, what will be the concentration of Na+ ? (a) 0.10M (b) 0.80M (c) 0.20M (d) 0.40M...

You have a 5 mL sample of a protein in 0.5 M NaCl. You place the...

You have a 5 mL sample of a protein in 0.5 M NaCl. You place the protein/salt sample inside dialysis tubing (see below) and place the bag in a large beaker of distilled water. If your goal is to remove as much NaCl from the sample as possible, which would be more effective: (1) placing the dialysis bag in 4 L of distilled water for 12 h, or (2) placing the bag in 1 L of distilled water for 6...

determine the pH of each two component solution a.) 0.550 M HI and 0.850 M HF...

determine the pH of each two component solution a.) 0.550 M HI and 0.850 M HF b.) 0.112 M NaCl and 0.953 M HF c.) 0.050 M KOH and 0.015 M Ba(OH)2 d.) 0.088 M HClO4 and 0.022 M KOH

You have 420 mL of an aqueous solution that is 0.39 M Na2SO4 and a separate...

You have 420 mL of an aqueous solution that is 0.39 M Na2SO4 and a separate 185 mL aqueous solution that is 0.45 M BaCl2. a). How many moles of each of the four ions are present ? Na+ SO42- Ba2+ Cl- b). When these two solutions are mixed together, what is the chemical formula of the solid expected to precipitate from the mixture? c). If the sulfate ions in the mixed solution react with the barium ions in the...

In the laboratory, a general chemistry student measured the pH of a 0.550 M aqueous solution...

In the laboratory, a general chemistry student measured the pH of a 0.550 M aqueous solution of formic acid, HCOOH to be 1.987. Use the information she obtained to determine the Ka for this acid. Ka(experiment) =

You have 15.00 mL of a 0.150 M aqueous solution of the weak base C5H5N (Kb...

You have 15.00 mL of a 0.150 M aqueous solution of the weak base C5H5N (Kb = 1.50 x 10-9). This solution will be titrated with 0.150 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 5.00 mL of acid has been added? (d) What is the pH of the solution...

You have 25.00 mL of a 0.250 M aqueous solution of the weak base CH3NH2 (Kb...

You have 25.00 mL of a 0.250 M aqueous solution of the weak base CH3NH2 (Kb = 5.00 x 10-4). This solution will be titrated with 0.250 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 5.00 mL of acid has been added? (d) What is the pH of the solution...

When 50.0 mL of aqueous 0.306 M (NH4)2CO3 and 50.0 mL of aqueous 0.229 M AlCl3...

When 50.0 mL of aqueous 0.306 M (NH4)2CO3 and 50.0 mL of aqueous 0.229 M AlCl3 are mixed together, what is the mass in grams of solid formed? Show your work in the space below

5. You have a dialysis bag containing 15-mL protein solution in 0.20 M NaCl. a. Would...

5. You have a dialysis bag containing 15-mL protein solution in 0.20 M NaCl. a. Would it be more efficient to dialyse this solution against i)one 2 L volume of buffer until equilibrium is reached, or to ii)dialyze the solution against one L buffer until equilibrium is reached, the remove the bag and dialyze against another one L of buffer til equilibrium is reached. Assume there is no volume change in the dialysis bag with dialysis. (1 pt) {type answer...

Question