Chemistry, 13.07.2019 00:30, jazare05

Let us assume that fe(oh)2(s) is completely insoluble, which signifies that the precipitation reaction with naoh(aq) (presented in the transition) would go to completion. fe2+(aq)+2naoh(aq) → fe(oh)2(s)+2na+(aq) if you had a 0.500 l solution containing 0.0230 m of fe2+(aq), and you wished to add enough 1.29 m naoh(aq) to precipitate all of the metal, what is the minimum amount of the naoh(aq) solution you would need to add? assume that the naoh(aq) solution is the only source of oh−(aq) for the precipitation.

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The study of chemicals and bonds is called chemistry. There are two types of solution and these are the acidic and basic solutions.

The correct answer to the question is 17.8ml of NaOH.

What is a chemical equation?A chemical equation is the symbolic representation of a chemical reaction in the form of symbols and formulae,

The chemical equation is as follows:-

$Fe^{2+} + 2NaOH --- Fe(OH)_2 + 2Na^+$

The moles of $Fe^{2+$ is as follows:-

Moles of $Fe^{2+} = 500 mL Fe^{2+} * \frac{0.0230mole\ Fe^{2+}]}{[1 mol\ Fe^{2+}}$ = 11.50 mmol Fe^(2+)

The moles of NaOH is as follows;-

Moles of NaOH = $11.50\ mmol\ Fe^{2+} * \frac{[2 \ mol\ NaOH]}{[1 \mol Fe^{2+}}$ = 23.00 mmol NaOH

The volume of NaOH is as follows:-

Volume of NaOH = $23.00 mmol NaOH * \frac{1 \ mL NaOH}{1.29 mmol NaOH}$ = 17.8 mL NaOH.

hence, the correct answer is 17.8

For more information about the moles, refer to the link:-

link

answered: babygirlgabby2137

17.8 mL NaOH

Step 1. Write the chemical equation

Fe^(2+) + 2NaOH → Fe(OH)2 + 2Na^(+)

Step 2. Calculate the moles of Fe^(2+)

Moles of Fe^(2+) = 500 mL Fe^(2+) × [0.0230 mmol Fe^(2+)]/[1 mL Fe^(2+)]

= 11.50 mmol Fe^(2+)

Step 3. Calculate the moles of NaOH

Moles of NaOH = 11.50 mmol Fe^(2+) × [2 mmol NaOH]/[1 mmol Fe^(2+)]

= 23.00 mmol NaOH

Step 4. Calculate the volume of NaOH

Volume of NaOH = 23.00 mmol NaOH × (1 mL NaOH/1.29 mmol NaOH)

= 17.8 mL NaOH

answered: Guest

Afraidsugar lol it’s the third one

answered: Guest

remember that hf is only the energy of one photon. not two. not three. one. 1) 5.12 * 10^3 photons find the energy of one photon, then determine how many photons are needed to reach the sensitivity. e = hf = (6.626 * 10^-34 js)(5.95 * 10^19 hz) = 3.94247 * 10^-14 j per photon (2.02 * 10^-10 j) / (3.94247 * 10^-14 j/photon) = 5123.69149 photons round to three sig figs. 2) 5.77 * 10^-17 j energy of pulse = energy per photon * number of photons = hfn = (6.626 * 10^-34 js)(1.66 * 10^13 hz)(5250) = 5.774559 * 10^-17 j round to three sig figs. 3) 4.07 * 10^8 kj/mol 10^12 pm = 1 m c = fλ f = c/λ e = hf = hc/λ = [(6.626 * 10^-34 js)(3.00 * 10^8 m/s) / (2.94 * 10^-12 m)](1 kj/1000 j)(6.02 * 10^23 photons/mol) = 40702571.4 kj/mol round to three sig figs. 4) 9.94 * 10^-1 m e = hc/λ λ = hc / e = (6.626 * 10^-34 js)(3.00 * 10^8 m/s) / (2.00 * 10^-25 j) = 0.9939 m round to three sig figs. 5) 9.06 * 10^3 photons energy of pulse = energy per photon * number of photons number of photons = energy of pulse / energy per photon = energy of pulse / (hf) = (3.87 * 10^-13 j) / [(6.626 * 10^-34 js)(6.45 * 10^16 hz)] = 9055.23695 photons round to three sig figs. 6) 2.78 * 10^-15 j this is problem 1, except in reverse. sensitivity = minumum number of photons * energy per photon = (5930)(6.626 * 10^-34 js)(7.077 * 10^14 hz) = 2.78070758 × 10^-15 j round to three sig figs.