What are the major species present in a 0.150-M NH3 solution? Calculate the [OH2] and the...

What are the major species present in a 0.150-M NH3 solution? Calculate the [OH2] and the pH of this solution.

Solutions

Expert Solution

Since NH3 is weak base . A weak base con not ionize completely to prodcue NH4+ and OH-

So the major species are NH3 & H2O only.

To find the pH and conc of OH-

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

Calculate the pH and moralities of all the species in a 0.150 M ammonia solution. Ka...

Calculate the pH and moralities of all the species in a 0.150 M ammonia solution. Ka = 5.55 x 10-10

Calculate the concentration (in M) of each species present in a 0.085 M solution of H2GeO3....

Calculate the concentration (in M) of each species present in a 0.085 M solution of H2GeO3. (See the Acid and Base Dissociation Constants table. Assume Kw = 1.01 ✕ 10−14.) [H2GeO3]______ M [HGeO3− ]______ M [GeO32− ]______ M M [H3O+ ]______ M M [OH − ]_______ M

Calculate the concentration of all species in a 0.150 M solution of H2CO3. H2CO3], [HCO−3], [CO2−3],...

Calculate the concentration of all species in a 0.150 M solution of H2CO3. H2CO3], [HCO−3], [CO2−3], [H3O+], [OH−] = Enter your answers numerically separated by commas. Express your answer using two significant figures.

A solution is made by mixing 0.150 M NH4Cl and 0.100 M NH3. Ka for NH4+...

A solution is made by mixing 0.150 M NH4Cl and 0.100 M NH3. Ka for NH4+ is 5.61x10-10 (please show math) a. What type of solution you will have when the two compounds are mixed? b. Identify the acid and the base (write the formula and the ID next to it) c. Will Cl- affect the pH of the solution? Why? d. What is your prediction for the calculated pH compared to the pKa of the sample? Why? e. What...

Calculate the concentration of all species present in a 0.01 M aqueous solution of ammonia. The...

Calculate the concentration of all species present in a 0.01 M aqueous solution of ammonia. The pKa of the ammonium ion is 9.24. 1)Calculate [H+] (express the result in molar units using three significant figures and scientific notation). 2)Calculate [OH-] (express the result in molar units using three significant figures and scientific notation). 3)Calculate [NH+4] (express the result in molar units using three significant figures and scientific notation). 4)Calculate [NH3] (express the result in molar units using three significant figures...

Calculate the concentration of all species present in a 0.01 M aqueous solution of ammonia. The...

Calculate the concentration of all species present in a 0.01 M aqueous solution of ammonia. The pKa of the ammonium ion is 9.24. A.)Calculate [H+] (express the result in molar units using three significant figures and scientific notation). B.)Calculate [OH-] (express the result in molar units using three significant figures and scientific notation). C.)Calculate [NH+4] (express the result in molar units using three significant figures and scientific notation). D.)Calculate [NH3] (express the result in molar units using three significant figures and scientific...

1.A solution is made by mixing 0.150 M NH4Cl and 0.100 M NH3. Ka for NH4+...

1.A solution is made by mixing 0.150 M NH4Cl and 0.100 M NH3. Ka for NH4+ is 5.61x10-10 a.What type of solution you will have when the two compounds are mixed? b.Identify the acid and the base (write the formula and the ID next to it) c.Will Cl- affect the pH of the solution? Why? d.What is your prediction for the calculated pH compared to the pKa of the sample? Why? e.What is the pH of the solution? Was your...

Calculate the concentrations of all five chemical species present in a 0.750 M solution of hypoiodous...

Calculate the concentrations of all five chemical species present in a 0.750 M solution of hypoiodous acid.

Calculate the ph of a solution that is 0.30 M in ammonia (NH3) and 0.20 M...

Calculate the ph of a solution that is 0.30 M in ammonia (NH3) and 0.20 M in ammonium chloride. Kb=1.76 x 10^-5 Then calculate the ph if you add 10 mL of 1.0 M HCl to 50 mL of your solution in the problem above.

A 30.00 mL solution of 0.235 M CH2NH2 was titrated with 0.150 M H2SO4. a) Calculate...

A 30.00 mL solution of 0.235 M CH2NH2 was titrated with 0.150 M H2SO4. a) Calculate the pH of the 30.00 mL solution of 0.235 M CH2NH2 b) Calculate the volume of 0.150 M H2SO4 required to neutralize the 30 mL solution of 0.235 M CH2NH2. c) Calculate the volume of 0.150 M H2SO4 required to neutralize half the mole of CH2NH2 present 30 Ml solution of 0.235 M CH2NH2 d) Calculte the pH of the solution in (c). e)...

Subjects