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shtirl [24]
3 years ago
10

Giovanni created this chart to study for an exam.

Chemistry
2 answers:
Olegator [25]3 years ago
7 0
Calcium carbonate is indeed used as an antacid (among Mg(OH)2, Al2(OH)3 and NaHCO3).

Ferrous oxide or Iron (II) oxide is a dark substance, and I would certainly think twice before using a dark tooth paste (Yew! ) It might even rust if left in the mouth for some time!

max2010maxim [7]3 years ago
7 0
<h3><u>Answer;</u></h3>

B) Swap the uses for iron oxide and calcium carbonate.

<h3><u>Explanation;</u></h3>
  • Calcium carbonate is a compound that is naturally found in marble, chalk and limestone. It is used in pharmaceutical applications as a cost <u>effective dietary calcium supplement, and also used in antacids.</u>
  • Calcium carbonate is also found in <u>products such as baking powder, tooth paste, and wine among others.</u>
  • Iron oxides are compounds of iron that are<u> used as coloring agents in some cosmetics.</u> The forms of iron oxides used in cosmetics are normally synthetic.
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If an atom gains an electron, what overall charge will it have?
Oliga [24]

Answer:

The atom will have a negative charge.

Explanation:

Electrons are subatomic particles with a negative charge, protons are subatomic particles with a negative charge, and neutrons have no charge. When a neutral atom's balance is disrupted by an extra electron, the atom  becomes negatively charged.

4 0
3 years ago
Read 2 more answers
a water sample is found to have a cl- content of 100ppm as nacl what is the concentration of chloride in moles per liter
ladessa [460]

Answer:

The concentration of chloride ion is 2.82\times10^{-3}\;mol/L

Explanation:

We know that 1 ppm is equal to 1 mg/L.

So, the Cl^- content 100 ppm suggests the presence of 100 mg of Cl^- in 1 L of solution.

The molar mass of Cl^- is equal to the molar mass of Cl atom as the mass of the excess electron in Cl^- is negligible as compared to the mass of Cl atom.

So, the molar mass of Cl^- is 35.453 g/mol.

Number of moles = (Mass)/(Molar mass)

Hence, the number of moles (N) of Cl^- present in 100 mg (0.100 g) of Cl^- is calculated as shown below:

N=\frac{0.100\;g}{35.453\;g/mol}=2.82\times 10^{-3}\;mol

So, there is 2.82\times10^{-3}\;mol of Cl^- present in 1 L of solution.

5 0
3 years ago
Determine the number of moles of gas in a 4.1L container at 341K with a pressure of 1.78 atm.
lozanna [386]

Answer:

0.26 mol

Explanation:

using general gas equation

PV=nRT

V=4.1litre= 4.1 dm³

P= 1.78 atm

R= 0.0821

PUT VALUES

8 0
3 years ago
Suppose of potassium iodide is dissolved in of a aqueous solution of silver nitrate. Calculate the final molarity of iodide anio
Sholpan [36]

The given question is incomplete, the complete question is:

Suppose 1.27 g of potassium iodide is dissolved in 100. mL of a 44.0 m M aqueous solution of silver nitrate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of the solution doesn't change when the potassium iodide is dissolved in it. Round your answer to 3 significant digits.

Answer:

The correct answer is 0.0325 M.

Explanation:

The mass of potassium iodide or KI mentioned in the question is 1.27 grams, the molar mass of KI is 166 g/mol. The formula for determining the no of moles of the substance is mass/molar mass. Thus, the moles of KI in 1.27 grams will be,  

= 1.27g / 166 g/mol = 0.00765 moles.  

KI = K⁺ + I⁻

Therefore, the moles of KI will be equivalent to moles of iodide anion, that is, 0.00765 moles.  

The moles of silver nitrate or AgNo3 in the solution can be determined by using the formula, molarity (M) * volume in liters. The molarity of silver nitrate given in the question is 44 mM and the volume used is 100 ml or 100/1000 L. Now putting the values we get,  

= (44 M/1000) * (100 L/1000) = 0.0044 moles

The moles of silver nitrate is equivalent to moles of silver ion, which is further equivalent to the moles of iodide ion that has taken part in precipitation = 0.0044 moles.  

The moles left of I⁻ in the solution will be,  

0.00765 - 0.0044 = 0.00325

Now, the final molarity of iodide ion in the solution will be,  

= moles/volume in liters

= 0.00325 moles / 0.100 L = 0.0325 M

7 0
3 years ago
Oceanic crust
ludmilkaskok [199]

Answer: It would be C

7 0
3 years ago
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