Questions LLC
Login
or
Sign Up
Ask a New Question
Chemistry
Solutions and Solubility
Van't Hoff factor
Calculate the van't Hoff factor for a solute that is a univalent-univalent weak electrolyte and is 25% ionized.
a. 15.0
b. 1.75
c. 1.25
d. 122
1 answer
% ionization = (i – 1) × 100%
You can
ask a new question
or
answer this question
.
Similar Questions
Identify the solute with the highest van't Hoff factor: Non-electrolyte, NaCl, MgCl2, FeCl3, MgSO4
Top answer:
fecl3
Read more.
1. Van't Hoff factors depend on the concentrations of the dissolved solute species. Why would a dilute solution have a Van't
Top answer:
1. http://www.chemguide.co.uk/physical/phaseeqia/nonideal.html 2. C = KpP Plug in K and P and solve
Read more.
Is the experimental Van't Hoff factor for ionic molecules always higher or lower than the theoretical Van't Hoff factor? Why?
Hig
Top answer:
The correct answer is: Lower, because of the dynamic equilibrium between the ions dissolved in the
Read more.
How does the van't hoff factor relate to freezing points? If one van't hoff factor is bigger than another, is its freezing point
Top answer:
Ah, the van't Hoff factor and freezing points! They're like two peas in a pod, but with a hilarious
Read more.
Can't figure out part 2/3
1) If the osmotic pressure of a 3.62×10-2-M aqueous solution of Ca(NO3)2 was found to be 2.51 atm at
Top answer:
1. pi = iMRT. pi = i*0.0362*0.0821*293 = 2.51 i = 2.88 2. dT = i*Kf*m delta T = 2.88*1.86*0.0365
Read more.
What is the Van't Hoff Factor of
MgSO4*7H2O? We're doing a colligative properties lab at my school where we dissolve various
Top answer:
I would expect two. You have two ions in solution, the magnesium ion, and the sulfate ion.
Read more.
A 1.00% by mass MgSO4 solution has a freezing point of -.192°C. Water has a Kf of 1.86 (KxKg)/mol.
a.) Estimate the van’t Hoff
Top answer:
To calculate the total molality of all solute species, you need to consider the moles of each
Read more.
If an 0.650 m aqueous solution freezes at –2.00 °C, what is the van't Hoff factor, i, of the solute? Kf values can be found
Top answer:
delta T = i*Kf*m 2.00 = i*1.86*0.650 i = (2.00/1.86*0.65) = ? I obtained 1.65 for i.
Read more.
Can someone confirm that I'd be doing this right?
If an 0.520 m aqueous solution freezes at -3.00 C, what is the van't Hoff
Top answer:
got it thank you to anyone who may have given thought!
Read more.
The boiling point of an aqueous 1.83 m salt solution is 102.5°C. Determine the value of the van't Hoff factor for this solute
Top answer:
delta T = i*Kb*m Substitute and solve for i.
Read more.
Related Questions
20) The ideal value of i (van't Hoff factor) for (NH4)3PO4.
A) 2 B) 5 C) 4 D) 3 E) 1 I know the answer but how are problems like
compare table salt with glucose
table salt is a strong electrolyte that will completely dissolve in a solution. whereas, glucose
What is the van't Hoff factor for K2SO4 in an aqueous solution that is 5.00 % K2SO4 by mass and freezes at -1.21 ∘C?
Which of the following is a weak electrolyte in aqueous solution?
a. H2SO3 b. HNO3 c. HBr d. HClO4 e. NaOH
Calculate the boiling point elevation of a solution made from 15.0 g of a nonelectrolyte solute and 250.0 g of water. the molar
A dilute electrolyte is not necessary weak and a concentrated electrolyte weak and a concentrated electrolyte is necessary
A 0.98 m aqueous solution of an ionic compound with the formula MX has a freezing point of -2.6∘C Calculate the van't Hoff
I keep thinking that 3 is the van't hoff factor for ammonium chloride, but I keep getting my answer wrong. Any ideas?
At what temperature would a 1.75m NaCl solution freeze, given that the van't Hoff factor for NaCl is 1.9? Kf for water is 1.86
Can you please tell me if these are right?
Classify the solutes in the following equations as a weak electrolyte, a strong