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horsena [70]
3 years ago
15

Kidney stones are caused by the precipitation of either calcium oxalate, Ca(C2O4), or calcium phosphate, Ca3(PO4)2, in the kidne

ys. If the normal concentration of Ca2+ in the kidneys is 2.5 mM, at what concentration of oxalate ion will kidney stones begin to form?
Chemistry
1 answer:
krek1111 [17]3 years ago
3 0

Answer:

1.1 × 10⁻⁶ M

Explanation:

Step 1: Given and required data

  • Concentration of Ca²⁺ ([Ca²⁺]): 2.5 mM = 2.5 × 10⁻³ M
  • Calcium oxalate solubility product constant (Ksp): 2.7 × 10⁻⁹

Step 2: Write the balanced equation for the solution reaction of calcium oxalate

CaC₂O₄(s) ⇄ Ca²⁺(aq) + C₂O₄²⁻(aq)

Step 3: Calculate the concentration of the oxalate ion to begin the precipitation of calcium oxalate

We will use the Ksp of calcium oxalate.

Ksp = 2.7 × 10⁻⁹ = [Ca²⁺].[C₂O₄²⁻]

[C₂O₄²⁻] = Ksp / [Ca²⁺]

[C₂O₄²⁻] = 2.7 × 10⁻⁹ / 2.5 × 10⁻³

[C₂O₄²⁻] = 1.1 × 10⁻⁶ M

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Answer:

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Explanation:

2CH_{4(g)} +3O_{2(g)} -->2CO(g)+4H_{2}O_{(g)}\\CH_{4(g)} +2O_{2(g)} -->CO_{2(g)} +2H_{2}O_{(g)} \\

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3 years ago
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8 0
3 years ago
Microwave radiation has a wavelength on the order of 1.0 cm. Calculate the frequency and the energy of a single photon of this r
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Answer :

(1) The frequency of photon is, 3\times 10^{10}Hz

(2) The energy of a single photon of this radiation is 1.988\times 10^{-23}J/photon

(3) The energy of an Avogadro's number of photons of this radiation is, 11.97 J/mol

Explanation : Given,

Wavelength of photon = 1.0cm=0.01m     (1 m = 100 cm)

(1) Now we have to calculate the frequency of photon.

Formula used :

\nu=\frac{c}{\lambda}

where,

\nu = frequency of photon

\lambda = wavelength of photon

c = speed of light = 3\times 10^8m/s

Now put all the given values in the above formula, we get:

\nu=\frac{3\times 10^8m/s}{0.01m}

\nu=3\times 10^{10}s^{-1}=3\times 10^{10}Hz    (1Hz=1s^{-1})

The frequency of photon is, 3\times 10^{10}Hz

(2) Now we have to calculate the energy of photon.

Formula used :

E=h\times \nu

where,

\nu = frequency of photon

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Now put all the given values in the above formula, we get:

E=(6.626\times 10^{-34}Js)\times (3\times 10^{10}s^{-1})

E=1.988\times 10^{-23}J/photon

The energy of a single photon of this radiation is 1.988\times 10^{-23}J/photon

(3) Now we have to calculate the energy in J/mol.

E=1.988\times 10^{-23}J/photon

E=(1.988\times 10^{-23}J/photon)\times (6.022\times 10^{23}photon/mol)

E=11.97J/mol

The energy of an Avogadro's number of photons of this radiation is, 11.97 J/mol

3 0
3 years ago
Read 2 more answers
Does anyone know how to do this???
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The number of valence electrons that is given by the group that the element is in, the top number of each column in the periodic table.







8 0
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