A solution consists of 44.3 g of hydrochloric acid (HCl), 75.7 g water, and has a...

A solution consists of 44.3 g of hydrochloric acid (HCl), 75.7 g water, and has a volume of 101 mL.

Calculate the weight percent of HCl, the molality of HCl, the mole fraction of HCl, and the molarity of HCl in the solution.

weight percent =	%
molality =	m
mole fraction =
molarity =	M

A solution of barium chloride (BaCl₂) in water is 5.000 % barium chloride by mass. Its density is 1.0434 g cm^-3 at 20 °C. Compute its molarity, mole fraction, and molality at this temperature.

Molarity BaCl₂ =

Mole fraction BaCl₂ =

Molality BaCl₂ =

The EPA's secondary standards for contaminants that may cause cosmetic or aesthetic effects in drinking water suggest an upper limit of 5.00×10^-2 mg/L for manganese . If 1.40×10⁴ liters of water in a storage tank contains 2.66 grams of Mn, what is the contaminant level in ppm? Is this level acceptable based on EPA guidelines?

ppm _________acceptable/not acceptable

Expert Solution

queen_honey_blossom answered 9 months ago

A) An aqueous solution is 3.50% by mass hydrochloric acid, HCl, and has a density of...

A) An aqueous solution is 3.50% by mass hydrochloric acid, HCl, and has a density of 1.02 g/mL. The molality of hydrochloric acid in the solution is ____ m. B) An aqueous solution of iron(III) sulfate has a concentration of 0.192 molal. The percent by mass of iron(III) sulfate in the solution is ____ %.

Concentrated hydrochloric acid solution is 37.0% HCL and has a density of 1.19g/ml. A dilute solution...

Concentrated hydrochloric acid solution is 37.0% HCL and has a density of 1.19g/ml. A dilute solution of HCL is prepared by diluting 4.50mL of this acid to 100.00mL with water. Then 10.0mL of the dilute HCL is used for the reaction with AgNO3 solution as shown below: HCL(aq)+AgNO3(aq) to HNO3(aq)+AgCL(s) How many mL of 0.1105M AgNO3 solution is required to precipitate all of the chloride as AgCl(s)? Please show how you get the answer. Thank you!

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How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL) are required to produce 20.0 L of a solution that has a pH of 1.80?

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Hydrochloric acid is produced by absorbing gaseous HCl (hydrogen chloride) in water. Calculate the heat that...

Hydrochloric acid is produced by absorbing gaseous HCl (hydrogen chloride) in water. Calculate the heat that must be transferred to or from an absorption unit if HCl(g) at 100°C and H2O(l) at 25°C are fed to produce 1000 kg/h of 20 wt% HCl(aq) at 40°C. Assume the heat capacity of the produced HCl is 0.557 kJ/mol HCl .°C

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Consider the combustion of hydrochloric acid. 4 HCl (aq) + O2(g)  2H2O(l) + 2 Cl2(g)...

Consider the combustion of hydrochloric acid. 4 HCl (aq) + O2(g)  2H2O(l) + 2 Cl2(g) ΔHrxn = + 96.976 kJ/mol B.If you place 750 mL of 0.500 M solution of HCl with 17.2 g of O2, will any oxygen remain? (Hint: limiting reagent problem) C.What mass of chlorine gas (in grams) is produced? D) How many molecules of Cl2 are produced based on part (B) E) What mass of excess reagent remains after the limiting reagent is used up?...

Hydrochloric acid (HCl) reacts with sodium carbonate (Na2CO3), forming sodium chloride (NaCl), water (H2O), and carbon...

Hydrochloric acid (HCl) reacts with sodium carbonate (Na2CO3), forming sodium chloride (NaCl), water (H2O), and carbon dioxide (CO2). This equation is balanced as written: 2HCl(aq)+Na2CO3(aq)→2NaCl(aq)+H2O(l)+CO2(g) Part A: What volume of 2.75 M HCl in liters is needed to react completely (with nothing left over) with 0.750 L of 0.400 M Na2CO3? Part B: A 675-mL sample of unknown HCl solution reacts completely with Na2CO3 to form 18.1 g CO2. What was the concentration of the HCl solution?

When 200. mL of 0.40 M hydrochloric acid solution is mixed with 3.76 g of aluminum...

When 200. mL of 0.40 M hydrochloric acid solution is mixed with 3.76 g of aluminum metal, how many moles of hydrogen gas would be produced? 6HCl(aq) + 2Al(s) → 2AlCl3(aq) + 3H2(g)

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