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Marizza181 [45]

3 years ago

8

The slight negative charge at one end of one water molecule is attracted to the slight positive charge of another water molecule

. What is this attraction called?
A. A covalent bond
B. Hydrogen bond
C.an ionic bond
D. a hydrophilic bond
E. A hydrophobic bond

2 answers:

Liono4ka [1.6K]3 years ago

8 0

Your answer is <em>B </em>or<em> hydrogen bond. ;)</em>

Novay_Z [31]3 years ago

3 0

B hydrogen bond i think

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A mass of one centigram is a mass of<br><br> A 100g<br><br> B 10 g<br><br> C .01 g<br><br> D 1000 g

____ [38]

Mass of 1 centigram is equal to 0.01 grams
So, option C is your answer!

Hope this helps!

4 0

3 years ago

Read 2 more answers

An antacid tablet was dissolved in water and 10mL of 0.16M HCl was added. After the acid had reacted with the tablet it required

Mnenie [13.5K]

Answer:

0.0008 mole of HCl

Explanation:

From the balanced equation between HCl and NaOH:

$HCl + NaOH --> NaCl + H_2O$

1 mole of acid requires 1 mole of base for neutralization.

mole = molarity x volume

mole of NaOH = 0.02 x 0.04 = 0.0008 mole

mole HCl = 0.16 x 0.01 = 0.0016 mole

Since 1 mole of NaOH requires 1 mole of HCl for neutralization, it means that 0.0008 mole of NaOH will require 0.0008 mole of HCl. The remaining mole of HCl must have been neutralized by the antiacid:

0.0016 - 0.0008 = 0.0008 mole.

Therefore, 0.0008 mole of HCl must have been neutralized by the antiacid.

7 0

4 years ago

2KCIO3 ----------> 2KCI + 302<br> How many moles of KCIO3 are needed to make 3.5 moles of KCL?

lyudmila [28]

Answer:

3.5 mol KClO3

Explanation:

Given 3.50 moles of KCl as the target amount in the problem, used the coefficient of the balanced chemical reaction involved to determine the number of moles of potassium perchlorate needed.

x mole of KClO3 = 3.5 mol KCl x [(2 mol KCl)/ (2 mol KClO3)] = 3.5 mol KClO3

x mole of KClO3 = 3.5 mol KClO3

3 0

3 years ago

During a lab, you heat 1.62 g of a CoCl2 hydrate over a Bunsen burner. After heating, the final mass of the dehydrated compound

sashaice [31]

Answer is: formula of hydrate is CoCl₂· 6H₂O -c<span>obalt(II) chloride hexahydrate
</span>m(CoCl₂· xH₂O) = 1,62 g.
m(CoCl₂) = 0,88 g.
n(CoCl₂) = m(CoCl₂) ÷ M(CoCl₂)
n(CoCl₂) = 0,88 g ÷ 130 g/mol
n(CoCl₂) = 0,0068 mol.
m(H₂O) = 1,62 g - 0,88 g.
m(H₂O) = 0,74 g.
n(H₂O) = m(H₂O) ÷ m(H₂O)
n(H₂O) = 0,74 g ÷ 18 g/mol
n(H₂O) = 0,041 mol.
n(CoCl₂) : n(H₂O) = 0,0068 mol : 0,041 mol.
n(CoCl₂) : n(H₂O) = 1 : 6.

8 0

3 years ago

1. Calculate how many moles of glycine are in a 130.0-g sample of glycine.2. Calculate the percent nitrogen by mass in glycine.

Alexxx [7]

Answer:

$n=1.732mol$

$\% N=18.7\%$

Explanation:

Hello!

In this case, since the molecular formula of glycine is C₂H₅NO₂, we realize that the molar mass is 75.07 g/mol; thus, the moles in 130.0 g of glycine are:

$n=130.0g*\frac{1mol}{75.07 g}\\\\ n=1.732mol$

Furthermore, we can notice 75.07 grams of glycine contains 14.01 grams of nitrogen; thus, the percent nitrogen turns out:

$\% N=\frac{14.01}{75.07}*100\% \\\\\% N=18.7\%$

Best regards!

4 0

3 years ago