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soldier1979 [14.2K]
3 years ago
15

Which of the following best explains how water is able to dissolve ionic substances?

Chemistry
2 answers:
NikAS [45]3 years ago
8 0

Answer: The positive and negative charges of the water molecule pull on the negative and positive ends of the ionic molecule to break them apart.

Explanation:  

Ionic compounds dissolve in polar solvents such as water as like dissolves like. Ionic compounds are made up of ions which remain attracted by coloumbic forces.  

Thus to separate the ions, the positive and negative charges of polar solvent pulls the opposite charges of the ionic compounds and thus break them apart. Thus the ionic compounds dissolve in water.



yanalaym [24]3 years ago
7 0
The correct answer to this question is "The positive and negative charges of the water molecule pull on the negative and positive ends of the ionic molecule to break them apart." This best explains how water is able to dissolve ionic substances. Thank you for posting your question. I hope that this answer helped you. Let me know if you need more help. 
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If the solvent is a liquid, then the solute:
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How will adding NaCl affect the freezing point of a solution?
lord [1]

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3 0
3 years ago
Read 2 more answers
determine mass of water formed when 12.5 L NH3(at298K and 1.50atm) is reacted with 18.9L of O2 (at 323K and 1.1atm)
sasho [114]

The  mass  of water formed  is


<u><em>calculation</em></u>

Use  the  ideal   gas  equation   to  calculate the  moles of  NH3  and O2

that  is  Pv= n RT

where;  P= pressure,  

V=  volume,

n = number  of  moles,

R=gas   constant  = 0.0821  l .atm/ mol.K

make n the formula of  the subject  by diving   both side  by  RT

n =  PV /RT

The   moles of NH3

n= (1.50 atm  x 12.5 L) /(  0.0821 L. atm /mol.k   x 298 K)  =0.766  moles

The  moles  of  O2

=(1.1 atm  x 18.9  L) /  (  0.0821 L. atm/ mol.k   x 323 K) = 0.784  moles


write the reaction  between  NH3  and  O2

4 NH3  + 5 O2  →4 No  +6H2O


from  equation above  0.766  moles of NH3  reacted to produce  

0.766 x 6/4 =1.149 moles of H2O


0.784  moles of O2   reacted to  produce  0.784  x 6/5=0.9408  moles  of H20


since  O2  is totally  consumed, O2  is the limiting  reagent  and therefore  the  moles of H2O  produced=  0.9408  moles


mass  of  H2O  = moles x molar mass

 from  periodic table the  molar mass  of H2O  =  (1 x2)+16= 18  g/mol

mass = 18 g/mol  x 0.9408  moles= 16.93  grams


3 0
3 years ago
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