A 2.00 × 103 mL sample of 3.00 M HCl solution is treated with 4.29 g...

2.00

10³

mL sample of 3.00 M HCl solution is treated with 4.29 g of magnesium. Calculate the concentration of the acid solution after all the metal has reacted. Assume that the volume remains unchanged.

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

A 40.0 mL of 2.00 M Fe3+ (aq) solution are mixed with 60.0 mL of 3.00...

A 40.0 mL of 2.00 M Fe3+ (aq) solution are mixed with 60.0 mL of 3.00 M SCN- (aq) solution. What is the equibrium concentratio of FeSCN2+ (aq), if the complex formation constanst is 189 for the reaction: Fe3+(aq) + SCN- (aq) -----> FeSCN2+ (aq) , Kf=189

An aqueous solution is 2.00 M urea. The density of the solution is 1.029 g/ml. What...

An aqueous solution is 2.00 M urea. The density of the solution is 1.029 g/ml. What is the molality concentration of urea in the solution?

A student plans to neutralize a 10.00 mL sample of 2.00 M HCl with sodium carbonate....

A student plans to neutralize a 10.00 mL sample of 2.00 M HCl with sodium carbonate. Consider sig. figs. for all answers. A. Balance the following equation that signifies the above reaction: Na2CO3 + HCl -> NaCl + H2O + CO2 B. Calculate the number of moles of HCl involved in the reaction C. Calculate the number of moles of Na2CO3 required to neutralize the moles of HCl found in (b) D. Calculate the mass (in grams) of Na2CO3 required to...

A solution of HCl is prepared by diluting 25.0 mL of a 1.0 M HCl solution...

A solution of HCl is prepared by diluting 25.0 mL of a 1.0 M HCl solution with enough water to make 750 mL of HCl solution. (Show your work for all calculations!) a) What is the molarity of the HCl solution? b) What is the [H3O+] and the pH of the HCl solution? c) Write the balanced chemical equation for the reaction of HCl and Ba(OH)2 d) How many milliliters of the diluted HCl solution is required to completely react...

A 1.268 g sample of a metal carbonate, MCO33, was treated 100.00 mL of 0.1083 M...

A 1.268 g sample of a metal carbonate, MCO33, was treated 100.00 mL of 0.1083 M H22SO44, yielding CO22 gas and an aqueous solution of the metal sulfate. The solution was boiled to remove all of the dissolved CO22 and then was titrated with 0.1241 M NaOH. A 71.02 mL volume of the NaOH solution was required to neutralize the excess H22SO44. Start by writing a balanced chemical equation for this reaction. What's the identity of the metal? Give the...

A 1.268 g sample of a metal carbonate (MCO3)was treated with 100.00 mL of 0.1083 M...

A 1.268 g sample of a metal carbonate (MCO3)was treated with 100.00 mL of 0.1083 M sulfuric acid (H2SO4), yielding CO2 gas and an aqueous solution of the metal sulfate (MSO4). The solution was boiled to remove all the dissolved CO2 and was then titrated with 1.241×10−2 MNaOH. A 91.86 mL volume of NaOH was required to neutralize the excess H2SO4. A) What is the identity of the metal M? B) How many liters of CO2 gas were produced if...

A 0.204-g sample of a CO3 antacid is dissolved with 25.0 mL of 0.0981 M HCL....

A 0.204-g sample of a CO3 antacid is dissolved with 25.0 mL of 0.0981 M HCL. The hydrochloric acid that is not neutralized by the antacid is titrated to a bromophenol blue endpoint with 5.83 mL of 0.104 M NaOH. a) Determine the moles of base per gram in the sample.

9) An aqueous solution of HCl is 0.500 M. Its density is 1.20 g/mL. Calculate the...

9) An aqueous solution of HCl is 0.500 M. Its density is 1.20 g/mL. Calculate the molality of HCl in this solution. a) 0.417 m b) 0.424 m c) 0.430 m d) 0.500 m e) 0.600 m 10) The normal freezing point of benzene (C6H6) is 5.48°C. When 2.00 g of an unknown covalent compound is dissolved in 100.0 g of benzene, the freezing point of the resulting solution is 5.08°C. What is the molar mass of the unknown compound?...

A solution was produced by dissolving NH3 to give a 250. mL solution with 3.00 M...

A solution was produced by dissolving NH3 to give a 250. mL solution with 3.00 M NH3. a. What is the pH of this solution? pH = b. What mass of NH4Cl must be added to this solution to give a pH of 9.45? __ g c. If 40. mL of 2.0 M KOH was added to this solution, what will be the pH of this solution? pH = d. If 40. mL of 2.0 M KOH was added to...

If we mix 40.0 mL of 3.00 M Pb(NO3)2 (aq) with 20.0 mL of 2.00 x...

If we mix 40.0 mL of 3.00 M Pb(NO3)2 (aq) with 20.0 mL of 2.00 x 10-3 M NaI (aq), does PbI2 (s) precipitate from solution? I yes, calculate how many moles of PbI2 (s) precipitate and the values of [Pb2+], [I-], [NO3-], and [Na+] at 25 C at equilibrium?

Subjects