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umka21 [38]
3 years ago
9

Which best describe the tyndall effect

Chemistry
1 answer:
Svet_ta [14]3 years ago
6 0

The answer would be A

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What is the molarity of a solution containing 23 g of NaCl in 500 mL of solution?
trapecia [35]

molarity of a solution means mols per liter.

First, you need to convert 23 grams on NaCl into mols. 23g divided by molar mass (58.44g/mol) which gives you .394 mols.

Now, you need to convert 500ml to L which moves the decimal three places to the left, giving you .500L of solution.

Finally, divide the mols over solution to get .787M

7 0
2 years ago
Consider the equation below. Upper C a upper C upper O subscript 3 (s) double-headed arrow upper C a upper O (s) plus upper C up
stiks02 [169]

Answer:K subscript e q equals StartFraction StartBracket upper C upper O subscript 2 EndBracket StartBracket upper C a upper O EndBracket over StartBracket upper C a upper C upper O subscript 3 EndBracket EndFraction

Explanation: the answer has it's root in Law of mass action which states that; the rate of a chemical reaction is directly proportional to the product of the concentrations of the reactants raised to their respective stoichiometric coefficients.

8 0
3 years ago
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Convert 25.4 grams of barium phosphate, Ba3(PO4)2 to formula units.
Salsk061 [2.6K]
To solve this questions you first need to find the number of moles of barium phosphate you have. The molar mass of barium phosphate is 601.93g/mol.
24.4/601.83 = 0.0402 moles barium phosphate
Then you need to use avagadro’s number, 6.022 x 10^23, which is the number of molecules or formula units in a mole.

6.022 x 10^23 * 0.0402 = 2.42 x 10^22 formula units
7 0
2 years ago
On the basis of dipole moments and/or hydrogen bonding, explain in a qualitative way the differences in the boiling points of ac
Inga [223]
Go on google bro you can get more help there and hope you get what your looking for and good luck

7 0
3 years ago
Standard temperature and pressure are _____.
Maurinko [17]
The standard temperature is 0c.
the standard pressure is 1atm.
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3 years ago
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