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oksian1 [2.3K]
3 years ago
14

What is the term for a solid that forms when two solutions are mixed? a precipitate a gas a suspension a solution

Chemistry
2 answers:
SashulF [63]3 years ago
6 0
When a solid forms with two solutions are mixed it is a precipitate 
Oduvanchick [21]3 years ago
6 0

the term for a solid when two solutions are mixed is  a percipitate

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3 years ago
What is the GCF of 18 and 30
KengaRu [80]

Answer: it is 6

Explanation: your welcome

4 0
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Read 2 more answers
Identifying Characteristics of Atoms
Anon25 [30]

Explanation:

The number of protons in an atom is the atomic number.

Mass number is the number of protons plus neutrons in an atom.

  Mass number  = number of protons + number of neutrons

Atomic number  = number of protons

Atomic number gives the symbol of the element

Number        Number      Atomic      Mass          Symbol

 Protons       neutrons     Number    Number

     A                    7                 B              15                C

     D                   E                 26             56               F

A, number of protons  = B

 Mass number  = protons + neutrons

          15  = protons + 7

          Protons  = 15 - 7  = 8

Atomic number 8 is for oxygen = C

Atomic number  = number of protons  = D = 26

Number of neutrons ;

          E =    Neutrons  = mass number - protons  = 56  - 26  = 30

Atomic number 26 is for Iron = F

8 0
3 years ago
What is the pH of a 3.9•10-8 M OH- solution
Mice21 [21]
POH will be -log[conc of OH]
-log (3.9E-08) = 7.409
pH = 14- pOH
pH = 14 - 7.409
pH = 6.59
3 0
3 years ago
Convert 6.7 x 1024 molecules of nitrogen dioxide into grams.
BlackZzzverrR [31]

Answer:

510 g NO₂

General Formulas and Concepts:

  • Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.
  • Reading the Periodic Table
  • Writing Compounds
  • Using Dimensional Analysis

Explanation:

<u>Step 1: Define</u>

6.7 × 10²⁴ molecules NO₂ (Nitrogen dioxide)

<u>Step 2: Define conversions</u>

Avogadro's Number

Molar Mass of N - 14.01 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of NO₂ - 14.01 + 2(16.00) = 46.01 g/mol

<u>Step 3: Use Dimensional Analysis</u>

<u />6.7 \cdot 10^{24} \ molecules \ NO_2(\frac{1 \ mol \ NO_2}{6.022 \cdot 10^{23} \ molecules \ NO_2} )(\frac{46.01 \ g \ NO_2}{1 \ mol \ NO_2} ) = 511.901 g NO₂

<u>Step 4: Check</u>

<em>We are given 2 sig figs. Follow sig fig rules.</em>

511.901 g NO₂ ≈ 510 g NO₂

6 0
3 years ago
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