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1 year ago

Describe the three possible decisions you can receive from an

1 answer:

5 0

Answer 2. Accept with minor revisions: Also known as conditional acceptance, this decision means that the paper requires minor changes for it to be ...

wer:

Explanation:

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You are given an aqueous solution and are asked to analyze it for the presence (or absence) of Ag+(aq), Ca2+(aq), and/or Hg2+(aq

pantera1 [17]

Answer:

Explanation:

In the first step, hydrochloric acid (HCl) is added to the solution. In this case the equilibrium that could take place is:

Ag⁺(aq) + Cl⁻(aq) ↔ AgCl(s)

But no precipitate was formed, so Ag⁺(aq) is absent.

By adding H₂SO₄(aq) the next equilibrium that could take place is:

Ca⁺²(aq) + SO₄⁻²(aq) ↔ CaSO₄(s)

A white precipitate was formed, so Ca⁺² is present in the solution.

The following could take place after adding H₂S(aq):

Hg²⁺(aq) + S⁻² ↔ HgS(s)

A black precipitate formed, so Hg⁺² is present as well.

6 0

3 years ago

Which statement explains why a C–O bond is

Nataly_w [17]

Answer: (3) The difference in electronegativity between carbon and oxygen is greater than that between fluorine and oxygen.

Explanation: Polarity of a molecule is due to the difference in electronegativity of the atoms. More is the electronegativity difference, more is the polarity.

Electronegativity of carbon = 2.5

Electronegativity of oxygen = 3.5

Electronegativity of fluorine = 4.0

Thus the difference in electronegativity of carbon and oxygen is=(3.5-2.5)= 1.0

Thus the difference in electronegativity of fluorine and oxygen is=(4.0-3.5)= 0.5.

Thus C-O bond is more polar than F-O bond.

4 0

3 years ago

Read 2 more answers

A student dissolved 1.805g of a monoacidic weak base in 55mL of water. Calculate the equilibrium pH for the weak monoacidic base

yawa3891 [41]

Answer:

11.39

Explanation:

Given that:

$pK_{b}=4.82$

$K_{b}=10^{-4.82}=1.5136\times 10^{-5}$

Given that:

Mass = 1.805 g

Molar mass = 82.0343 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$Moles= \frac{1.805\ g}{82.0343\ g/mol}$

$Moles= 0.022\ moles$

Given Volume = 55 mL = 0.055 L ( 1 mL = 0.001 L)

$Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}$

$Molarity=\frac{0.022}{0.055}$

Concentration = 0.4 M

Consider the ICE take for the dissociation of the base as:

B + H₂O ⇄ BH⁺ + OH⁻

At t=0 0.4 - -

At t =equilibrium (0.4-x) x x

The expression for dissociation constant is:

$K_{b}=\frac {\left [ BH^{+} \right ]\left [ {OH}^- \right ]}{[B]}$

$1.5136\times 10^{-5}=\frac {x^2}{0.4-x}$

x is very small, so (0.4 - x) ≅ 0.4

Solving for x, we get:

x = 2.4606×10⁻³ M

pOH = -log[OH⁻] = -log(2.4606×10⁻³) = 2.61

5 0

2 years ago

What is the percent composition of Fluorine in CF5?

posledela

The answer is 100%
let me know if you want an explanation

6 0

2 years ago

Hard water often contains dissolved Ca2+ and Mg2+ ions. One way to soften water is to add phosphates. The phosphate ion forms in

katrin2010 [14]

Answer:

$22.4269$ grams of sodium phosphate must be added to 1.4 L of this solution to completely eliminate the hard water ions

Explanation:

We will first write the balanced equation for this scenario

3 CaCl2 + 2 Na3PO4 ----> 6 NaCl + Ca3 (PO4)2

3 Mg(NO3)2 + 2 Na3PO4 -----> 6 NaNO3 + Mg3 (PO4)2

The ratio here for both calcium chloride and magnesium nitrate is $3:2$

The number of moles of each compound is equal to

$0.054 * 1.4 = 0.0756\\0.093* 1.4 = 0.1302$

Using the mole ratio of 3:2, convert each to moles of sodium phosphate.

$0.0756$ mole of CaCl2 is equal to $0.05\\$ Na3PO4

$0.1302$ mole of CaCl2 is equal to $0.0868$ Na3PO4

Converting moles of sodium phosphate to grams of sodium phosphate we get

$(0.05 +0.0868) * 163.94$ g/mol

$22.4269$ grams of sodium phosphate must be added to 1.4 L of this solution to completely eliminate the hard water ions

8 0

3 years ago