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DaniilM [7]
2 years ago
5

Write the molecular formula of potassium chloride​

Chemistry
2 answers:
adell [148]2 years ago
6 0

Answer:

KCl

this is the answer hope its helps you I tried my best to give you the best answer ;)

Naddik [55]2 years ago
4 0

Answer:

KCl is the answers for the question

Explanation:

please give me brainlest

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Is carbon dioxide a pure substance
iVinArrow [24]

Answer:

It is not a pure substance.

6 0
3 years ago
If you have 120. mL of a 0.100 M TES buffer at pH 7.55 and you add 3.00 mL of 1.00 M HCl, what will be the new pH? (The pKa of T
Simora [160]

Answer:

The new pH after adding HCl is 7.07

Explanation:

The formula for calculating pH of a buffer is

pH = pKa + log([Conjugate base]/[Acid])

<u>Before adding HCl,</u>

         7.55 = 7.55 + log([Conjugate base]/[Acid])

⇔      log([Conjugate base]/[Acid])  = 0

⇔     [Conjugate base] = [Acid] = 1/2 x 0.100 = 0.05 M

⇒ Mole of Conjugate base = Mole of Acid = 0.05 M x 0.12 mL = 0.006 mol

<u>After adding HCl (3.00 mL, 1.00 M)</u>

⇒ Mole of HCl = 0.003 x 1 = 0.003 mol)

New volume solution is 120 m L+ 3 mL = 123 mL

HCl is a strong acid, it will convert the conjugate base to acid form, or we can express

Mole of new Conjugate base = 0.006 - 0.003 = 0.003 mol

                ⇒ Concentration = 0.003/0.123 M

Mole of new Acid form = 0.006 + 0.003 = 0.009 mol

                ⇒ Concentration = 0.009/0.123 M

Use the formula

pH = pKa + log([Conjugate base]/[Acid])

    = 7.55 + log(0.003 / 0.009) = 7.07

8 0
3 years ago
Hardness in groundwater is due to the presence of metal ions, primarily Mg2 and Ca2 . Hardness is generally reported as ppm CaCO
Maslowich

Answer:

  • 0.0144 M
  • 1440 ppm

Explanation:

Ca(In)²⁺ + EDTA → Ca(EDTA)²⁺ + In

We use the volume of EDTA consumed in the titration to <u>calculate the moles of Ca⁺² ions</u>:

  • 0.012 L * 0.0600 M * \frac{1molCa^{+2}}{1molEDTA} = 7.20x10⁻⁴ mol Ca⁺²

Now we <u>calculate the molarity</u>:

  • 7.20x10⁻⁴ mol Ca⁺² / 0.050 L = 0.0144 M

To calculate in ppm, we <u>use the moles of Ca⁺² and convert to mg of CaCO₃:</u>

  • 7.20x10⁻⁴ mol Ca⁺² = 7.20x10⁻⁴ mol CaCO₃
  • 7.20x10⁻⁴ mol CaCO₃ * 100g/mol * \frac{1000mg}{1g} = 72 mg CaCO₃

Finally, <u>the concentration in ppm</u> is:

  • 72 mg CaCO₃ / 0.050L = 1440 ppm
5 0
2 years ago
How can so many different substances in the world be made of so few elements?
Mrrafil [7]
Matematically speaking, maybe because:
The number of substances = number of elements + number of different combinations of those elements
7 0
3 years ago
Can you help me with this?
Nikitich [7]

Answer:

hi I'm sorry I can't I just need points

6 0
2 years ago
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