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lys-0071 [83]
3 years ago
15

0.25 L of aqueous solution contains 0.025g of HCLO4 (strong acid) what will be the Ph of the solution g

Chemistry
1 answer:
Elan Coil [88]3 years ago
4 0

Answer:

The pH of the solution will be 3

Explanation:

The strength of acids is determined by their ability to dissociate into ions in aqueous solution. A strong acid is any compound capable of completely and irreversibly releasing protons or hydrogen ions, H⁺. That is, an acid is said to be strong if it is fully dissociated into hydrogen ions and anions in solution.

Being pH=- log [H⁺] or pH= - log [H₃O⁺] and being a strong acid, all the HClO₃ dissociates:

HClO₄      +    H₂O        →      H₃O⁺      +      ClO₄-  

So: [HCLO₄]= [H₃O⁺]

The molar concentration is:

molar concentration=\frac{number of moles of solute}{volume solution}

The molar mass of HClO₄ being 100 g / mole, then if 100 grams of the compound are present in 1 mole, 0.025 grams in how many moles are present?

moles of HClO_{4} =\frac{0.025 grams*1 mole}{100 grams}

moles of HClO₄= 0.00025

Then:

[HClO_{4}]=\frac{0.00025 moles}{0.25 L}

[HClO_{4}]=0.001 \frac{ moles}{ L}

Being [HCLO₄]= [H₃O⁺]:

pH= - log 0.001

pH= 3

<u><em>The pH of the solution will be 3</em></u>

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

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3 0
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A 0.708 g sample of a metal, M, reacts completely with sulfuric acid according to the reaction M ( s ) + H 2 SO 4 ( aq ) ⟶ MSO 4
ollegr [7]

Answer:

The metal has a molar mass of 65.37 g/mol

Explanation:

Step 1: Data given

Mass of the metal = 0.708 grams

Volume of hydrogen = 275 mL = 0.275 L

Atmospheric pressure = 1.0079 bar = 0.9947 atm

Temperature = 25°C

Vapor pressure of water at 25 °C = 0.03167 bar = 0.03126 atm

Step 2: The balanced equation

M(s) + H2SO4(aq) ⟶ MSO4 (aq) + H2(g)

Step 3: Calculate pH2

Atmospheric pressure = vapor pressure of water + pressure of H2

0.9947 atm = 0.03126 atm + pressure of H2

Pressure of H2 = 0.9947 - 0.03126

Pressure of H2 = 0.96344 atm

Step 4: Calculate moles of H2

p*V=n*R*T

⇒ with p = The pressure of H2 = 0.96344 atm

⇒ with V = the volume of H2 = 0.275 L

⇒ with n = the number of moles H2 = TO BE DETERMINED

⇒ with R = the gas constant = 0.08206 L*atm/K*mol

⇒ with T = the temperature = 25°C = 298 Kelvin

n = (p*V)/(R*T)

n = (0.96344 * 0.275)/(0.08206*298)

n = 0.01083 moles

Step 5: Calculate moles of M

For 1 mole of H2 produced, we need 1 mole M

For 0.0108 moles of H2 we need 0.01083 moles of M

Step 6: Calculate molar mass of M

Molar mass M = Mass M / moles M

Molar mass M = 0.708 grams / 0.01083 moles

Molar mass M = 65.37 g/mol

The metal has a molar mass of 65.37 g/mol

5 0
3 years ago
5.36 litars of nitrogen gas are at :25°C and 733 mm Hg
ArbitrLikvidat [17]

Answer:

4.6L

Explanation:

Use the equation (P1*V1)/(T1)=(P2*V2)/(T2)

P= pressure

V= volume

T= temperature in kelvins (remember K= C + 273)

Convert atm to mmHg or vise versa

1.5atm*(760mmhg/1atm)= 1140mmHg

(733mmHg * 5.36L)/(298K)=(1140mmHg * V)/(402K)

V= 4.6 or 4.65L (depending on sig figs)

6 0
2 years ago
50 POINTS PLEASE HELP!
rjkz [21]

A physical change has occured, Boiling water is a physical change not a chemical one, now if you're talking about the electric current, that had not changes either. it may rearrange the molecules, but it does not change the fundamental properties of the substance.

5 0
3 years ago
Read 2 more answers
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