What must be the molarity of an aqueous solution of NH3 if it is 4.3 %...

What must be the molarity of an aqueous solution of NH3 if it is 4.3 % ionized? Express your answer using two significant figures.

Solutions

Expert Solution

queen_honey_blossom answered 1 month ago

Next > < Previous

Related Solutions

Calculate the molality, molarity,and mole fraction of NH3 in an 14.60 mass % aqueous solution (d...

Calculate the molality, molarity,and mole fraction of NH3 in an 14.60 mass % aqueous solution (d = 0.9651g/mL)

What is the molarity of a solution containing 13.7 grams of NH3 in 1.55 liters of...

What is the molarity of a solution containing 13.7 grams of NH3 in 1.55 liters of solution?

If some NH4Cl is added to an aqueous solution of NH3: A. the pH of the...

If some NH4Cl is added to an aqueous solution of NH3: A. the pH of the solution will decrease B. the solution will not have pH C. NH4Cl cannot be added to NH3 D. the pH of the solution will increase E. the pH of the solution will not change

The mole fraction of an aqueous solution of magnesium sulfite is 0.29. Calculate the molarity (in...

The mole fraction of an aqueous solution of magnesium sulfite is 0.29. Calculate the molarity (in mol/L) of the magnesium sulfite solution, if the density of the solution is 1.38 g mL-1. Determine the mole fraction of magnesium bromide in a 5.51 M aqueous solution of magnesium bromide. The density of the solution is 1.17 g mL-1.

The molar concentration of a 20.0% 9m/m) solution of aqueous ammonia (NH3) is 10.51 M. What...

The molar concentration of a 20.0% 9m/m) solution of aqueous ammonia (NH3) is 10.51 M. What is the density of this solution ?

a. Calculate the pH of a 0.538 M aqueous solution of ethylamine (C2H5NH2, Kb = 4.3×10-4)...

a. Calculate the pH of a 0.538 M aqueous solution of ethylamine (C2H5NH2, Kb = 4.3×10-4) b. Calculate the pH of a 0.0473 M aqueous solution of piperidine (C5H11N, Kb = 1.3×10-3).

find the pH of an aqueous 0.050 M carbonic acid (H2CO3) solution. Ka1 = 4.3 x...

find the pH of an aqueous 0.050 M carbonic acid (H2CO3) solution. Ka1 = 4.3 x 10^-7, Ka2 = 5.2 x 10^-11.

What mass of NH4Cl must be added to 250.0 mL of 0.200 M NH3 solution to...

What mass of NH4Cl must be added to 250.0 mL of 0.200 M NH3 solution to have a buffer solution at pH=8.90? Assume no volume change. A 15.0-mL sample of a H3PO4 solution is titrated with a 1.00 M NaOH solution. The neutralization reaction is complete when 33.6 mL of NaOH is added. What is the concentration of the H3PO4 solution (in M)?

1. A student prepares two aqueous solutions. For each solution: -Calculate the molarity. -Write a chemical...

1. A student prepares two aqueous solutions. For each solution: -Calculate the molarity. -Write a chemical equation representing the formation of the solution. Be sure to include phase labels and to show any ions that dissociate. -Draw a molecular picture of the solution showing any ions, solute molecules and water molecules. A. 2.91 g Na2CO3 to make 25.0 mL solution. B. 6.14 mL ethanol (d=0.789 g/mL) to make 75.0 mL of solution. C. Which solution is more concentrated? D. Identify...

what is the molarity? calculate the molarity of solution containing 0.652 mol of glucose C6h12o6 in...

what is the molarity? calculate the molarity of solution containing 0.652 mol of glucose C6h12o6 in 255000 g of water a solution contains 150.0 g of water (mw = 18.0 g/mol) and 50 g of ethanol (MW = 44.0 g/mol ) wat are the mole fraction of water and ethanol,and vapor pressure of the solution at 25 C (p water = 23.8 torr; p ethanol =58.7 torr)

Subjects