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Nesterboy [21]
3 years ago
14

Calculate the hydronium ion concentration in an aqueous solution with a pH of 11.7 at 25°C.

Chemistry
1 answer:
DENIUS [597]3 years ago
6 0

Answer:

Approximately 2\times 10^{-12}\;\rm mol \cdot L^{-1}.

Explanation:

The hydronium ion concentration \left[\mathrm{H_3O^{+}}\right] of an aqueous solution can be found from its \rm pH with the equation:

\displaystyle \left[\mathrm{H_3O^{+}}\right] = 10^{-\mathrm{pH}}.

For this solution, \rm pH= 11.7. Hence,

\begin{aligned}& \left[\mathrm{H_3O^{+}}\right] \\ &= 10^{-\mathrm{pH}} \\ &= 10^{-11.7} \approx 2 \times 10^{-12}\end{aligned}.

Note that for this equation, the number of significant figures in \left[\mathrm{H_3O^{+}}\right] should be the same as the number of decimal places in \rm pH. For example, the \rm pH of this question comes with only one decimal place. As a result, there would be only one significant figure in the \left[\mathrm{H_3O^{+}}\right] obtained from the equation.

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The boiling point of water is 100.00 °C at 1 atmosphere.
Oksana_A [137]

Answer:

The solution's boiling point is 100,2°C and its molality is 0,13 m

Explanation:

This is the colligative propertie about elevation of boiling point

ΔT = Kb . m . i where

ΔT is the difference between T° at boiling point of the solution - T° at boiling point of the solvent pure

Kb means ebulloscopic constant (<u><em>0,52 °C.kg/m .- a known value for water</em></u>)

m means molality (moles of solute in 1kg of solvent)

i means theVan 't Hoff factor ( degree of dissociation for a compound)

IT HAS NO UNITS

NiI2 ---> Ni2+  +  2I-  (we have 1 Ni2+ and 2 I-), the i for this, is 3

The 11,11 g of the salt are in 272,2g of water but I need to know how many mass of the salt is in 1000 g of water (1000 g is 1 kg) so the rule of three is:

272,2g ____ 11,11g

1000g _____ (1000 g . 11,11g) / 272,2g = 40,81g

As the molar mas of NiI2 is 312.5 g/mol, the moles of salt are, mass/molar mass, 40,81g /312.5 g/mol = 0,130 moles

T° of b p sl - 100°C = 0,52 °C.kg/m . 0,130 m/kg . 3

T° of boiling point solution = (0,52 °C.kg/m . 0,130 m/kg . 3) + 100°C

T° of boiling point solution = 100,2°C

4 0
3 years ago
A student attempts to measure the specific heat capacity of an unknown liquid through repeated trials. She measures its specific
Goryan [66]

Answer:

2.13

Explanation:

4 0
3 years ago
A functional group introduces heteroatoms into a carbon chain to increase
ivanzaharov [21]

Answer:

reactivaty

Explanation:

here you go for the answer

5 0
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What effect does increasing the concentration of a dissolved solute have on each of the colligative properties?
Igoryamba

Answer:

If we increase the concentration of a dissolved solute, the solution would have a vapor pressure so much low, the boiling temperature for the solution will be so high, freezing point for the solution will be so much low and the osmotic pressure will be higher.

Colligative properties always depends on dissolved particles (solute)

Explanation:

These are the colligative properties

- Vapor pressure lowering

ΔP = P° . Xm

Vapor pressure of pure solvent - Vapor pressure of solution.

If we add more solute, it would raise the Xm, so the solution would have a vapor pressure so much low.

Vapor pressure pure solvent - Vapor pressure solution ↑ = P° . Xm ↑

- Boiling point elevation

ΔT = Kb . m

When we add more solute, we are increasing the molality.

↑T° boiling of solution - T° boiling pure solvent = Kf . m ↑

Boiling temperature for the solution will be so high.

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When we add more solute, we are increasing the molality.

ΔT = Kf . m

T° fussion of pure solvent - ↓T° fussion of solution = Kf . m↑

Freezing point for the solution will be so much low.

- Osmotic pressure

π = M . R . T

When we add solute, molarity is increasing. Therefore the osmotic pressure will be higher.

π↑ = M↑ . R . T

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3 years ago
Which of the following is a chemical change
Oliga [24]

C. a burning candle

all the other choices are physical changes

3 0
3 years ago
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