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3 years ago

An unknown solution has a pH of 2 . How would you classify this solution?

Chemistry

2 answers:

o-na [289]3 years ago

7 0

Answer is: B. acidic.

pH (potential of hydrogen) is a numeric scale used to specify the acidity or basicity of an aqueous solution:

When pH is less than seven (pH<7), solution is acidic.

When is equal seven (pH = 7), solution is neutral.

When pH is greater than seven (pH > 7), solution is basic.

For example, hydrochloric acid( HCl) is acidic, it ionizes in water solution and gives the hydrogen cations and chloride anions (Cl⁻):

HCl(aq) → Cl⁻(aq) + H⁺(aq).

marin [14]3 years ago

7 0

B. ACIDIC :) pH<7 is considered to be acidic

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Calculate the ΔHrxn for the following

Vesnalui [34]

Answer:

2 NO (g) → N2 (g) + O2 (g)

2 NOCl (g) → 2 NO (g) + Cl2 (g)

____________________________

2NOCl (g) ⟶ N2 (g) + O2 (g) + Cl2 (g)

ΔH = [90.3 kJ x 2 x -1] + [-38.6 kJ x -1 x 2] = -103.4 kJ

The ΔH for the reaction is -103.4 kJ

6 0

3 years ago

When 32 grams of aluminum react, the actual yield is 105.5 grams, what is the percent yield?

user100 [1]

Answer:

329.7%

Explanation:

Percent Yield = Actual Yield/ Theoretical Yield x 100%

Percent Yield = 105.5g/32 x 100% = 329.69 ≈ 329.7 %

5 0

3 years ago

Complete combustion of a 0.600-g sample of a compound in a bomb calorimeter releases 24.0 kJ of heat. The bomb calorimeter has a

coldgirl [10]

The final temperature, t₂ = 30.9 °C

<h3>Further explanation</h3>

Given

24.0 kJ of heat = 24,000 J

Mass of calorimeter = 1.3 kg = 1300 g

Cs = 3.41 J/g°C

t₁= 25.5 °C

Required

The final temperature, t₂

Solution

Q = m.Cs.Δt

Q out (combustion of compound) = Q in (calorimeter)

24,000 = 1300 x 3.41 x (t₂-25.5)

t₂ = 30.9 °C

3 0

3 years ago

Read 2 more answers

How many moles of water contain 1.3 x 10^24 molecules?

Vika [28.1K]

C is the correct answer

3 0

3 years ago

What is the mass in grams of 0.000142 mol of vitamin c

bazaltina [42]

Answer:

0.0250 g

Explanation:

Step 1: Determine the molar mass of Vitamin C.

The molar mass is the mass in grams corresponding to 1 mole. In order to calculate the molar mass of vitamin C (C₆H₈O₆) we need to add the molar masses of the elements that compose it.

M(C₆H₈O₆) = 6 × M(C) + 8 × M(H) + 6 × M(O)

M(C₆H₈O₆) = 6 × 12.01 g/mol + 8 × 1.01 g/mol + 6 × 16.00 g/mol

M(C₆H₈O₆) = 176.14 g/mol

Step 2: Calculate the mass corresponding to 0.000142 mol of vitamin C.

$0.000142 mol \times \frac{176.14g}{mol} =0.0250 g$

7 0

3 years ago