Chemistry Middle School

If 45.0 mL of 0.25 M HCl is required to completely neutralize 25.0 mL of NH3, what is the concentration of the NH3 solution? Show all of the work needed to solve this problem.

HCl + NH3 yields NH4Cl

Answers

Answer 1

molar concentration = number of moles / volume  

number of moles = molar concentration × volume

Number of moles of HCl = 0.25 × 45 = 11.25 mmoles

From the reaction:

11.25 mmoles of HCl will neutralize 11.25 mmoles of NH₃

Molar concentration of NH₃ solution = 11.25 / 25 = 0.45 M

Answer 2

Answer:

The balanced chemical equation is

[tex]1HCl+1NH_3>1NH_4 Cl[/tex]

The conversions are  

Molarity of HCl and volume gives us moles HCl

Moles HCl to moles [tex]NH_3[/tex] (using mole ratio 1 : 1)

Moles [tex]NH_3[/tex] to Molarity [tex]NH_3[/tex]

Molarity  HCl = (moles solute HCl) / (volume of solution in L)

Rearranging the formula

We get moles HCl = Molarity × volume

[tex]=0.25M \times 45.0mL = 0.25 mol/L \times 0.045L = 0.01125 mol HCl[/tex]

moles HCl = moles [tex]NH_3[/tex] = 0.01125 mol [tex]NH_3[/tex]

Molarity  [tex]NH_3[/tex] =(moles solute [tex]NH_3[/tex]) / (volume of solution in L)

[tex]=\frac {(0.01125 mol )}{25.0mL} = \frac {(0.01125 mol )}{0.025L}[/tex]

=0.450 mol/L or M (Answer)

Related Questions

NF3 has three F atoms bonded to a central N atom, with one lone electron
pair on the N. What is the shape of this molecule?
O
A. Tetrahedral
O
B. Trigonal planar
O
C. Bent
O
D. Trigonal pyramidal

Answers

D Trigonal pyramidal

Explanation:

Final answer:

NF3 exhibits a trigonal pyramidal shape due to its sp³ hybridization, with three bonded fluorine atoms and one lone pair of electrons on the nitrogen atom.

Explanation:

The molecule in question is NF3, which consists of one nitrogen atom (N) and three fluorine atoms (F). The nitrogen atom in NF3 is sp³ hybridized, utilizing one sp³ hybrid orbital to form a bond with each of the three fluorine atoms, and the remaining sp³ hybrid orbital accommodates a lone pair of electrons. Considering the presence of three bonded pairs and one lone pair of electrons on the nitrogen atom, the molecular geometry of NF3 is trigonal pyramidal. This geometric shape resembles a tetrahedron with one vertex missing, due to the presence of the lone electron pair on nitrogen, which slightly distorts the angles between the bonds.

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