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Makovka662 [10]
2 years ago
6

Imagine you are working in the lab and your chemical bottle is labeled Fe2O3. Explain how you could

Chemistry
1 answer:
Sav [38]2 years ago
3 0
To determine the charge of the iron, you must know the charge from the oxygen. An oxygen ion has a -2 charge. Therefore, 3 oxygen ions have -6 charge. We know that charges must cancel out. If it were Fe+2 in the compound, the overall charge would be -2, which isn’t correct. So, we can conclude that it is Fe+3 found in iron (III) oxide.
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5 0
3 years ago
If the K a Ka of a monoprotic weak acid is 7.3 × 10 − 6 , 7.3×10−6, what is the pH pH of a 0.40 M 0.40 M solution of this acid?
olga_2 [115]

Answer:

pH =3.8

Explanation:

Lets call the monoprotic weak acid HA, the dissociation equilibria in water will be:

HA + H₂O   ⇄ H₃O⁺ + A⁻    with  Ka = [ H₃O⁺] x [A⁻]/ [HA]

The pH is the negative log of the H₃O⁺ concentration, we know the equilibrium constant, Ka and the original acid concentration. So we will need to find the [H₃O⁺] to solve this question.

In order to do that lets set up the ICE table helper which accounts for the species at equilibrium:

                          HA                                   H₃O⁺                          A⁻          

Initial, M             0.40                                   0                              0

Change , M          -x                                     +x                            +x

Equilibrium, M    0.40 - x                              x                               x

Lets express these concentrations in terms of the equilibrium constant:

Ka = x² / (0.40 - x )

Now the equilibrium constant is so small ( very little dissociation of HA ) that is safe to approximate 0.40 - x to 0.40,

7.3 x 10⁻⁶ = x² / 0.40  ⇒ x = √( 7.3 x 10⁻⁶ x 0.40 ) = 1.71 x 10⁻³

[H₃O⁺] = 1.71 x 10⁻³

Indeed 1.71 x 10⁻³ is small compared to 0.40 (0.4 %). To be a good approximation our value should be less or equal to 5 %.

pH = - log ( 1.71 x 10⁻³ ) = 3.8

Note: when the aprroximation is greater than 5 % we will need to solve the resulting quadratic equation.

4 0
3 years ago
Sodium metal (Na) reacts explosively with water to form sodium hydroxide (NaOH) and hydrogen gas. How many moles of sodium are n
Sati [7]

Answer:

308 moles of sodium

Explanation:

The balanced equation for the chemical reaction between sodium metal (Na) and water (H₂O) is the following:

2 Na(s) + 2 H₂O → 2 NaOH(aq) + H₂(g)

From the equation, we can see that 2 moles of Na react with 2 moles of H₂O to give 2 moles of NaOH and 1 mol of H₂ (hydrogen gas). So the stoichiometric mole ratio between Na and H₂ is: 2 mol Na/1 mol H₂. Thus, we multiply the mole ratio by the moles of H₂ to be produced to obtain the moles of Na required:

moles of Na required =  2 mol Na/1 mol H₂ x 154 moles H₂ = 308 moles Na

Therefore, 308 moles of sodium are needed to produce 154 moles of hydrogen gas.

7 0
3 years ago
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