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ddd [48]
2 years ago
12

What is the [Na2SO4] (MM = 142.04 g/mol) in ppt if 100.00 mL of a

Chemistry
1 answer:
Ugo [173]2 years ago
7 0

Answer:

1.345

Explanation:

I THINK SORRY

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Pretty sure its a mineral

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Beeswax is a naturally occurring wax secreted mainly by honeybees A. mellifera, for constructing honey combs (Tulloch, 1970a). Unhydrolyzed beeswax consists of approximately 71% esters, 15% hydrocarbons, 8% free fatty acids, and 6% other components (Tulloch, 1970b).

7 0
3 years ago
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Bari oxit có công thức hóa hóa học là BaO . vậy bari oxit được tạo nên từ các nguyên tố
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Bari oxit được tạo nên từ các nguyên tố Bari (Ba) và Oxi (O)

Explanation:

6 0
2 years ago
Absalon adds 1 g of salt to 1 L of room temperature water (25 °C). Then, he starts a timer and observes what happens. He notices
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I looked it up and found the answer lol

6 0
3 years ago
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For Na2HPO4:(( (Note that for H3PO4, ka1= 6.9x10-3, ka2 = 6.4x10-8, ka3 = 4.8x10-13 ) a) The active anion is H2PO4- b) The activ
Komok [63]

Answer:

Check the explanation

Explanation:

Answer – Given, H_3PO_4 acid and there are three Ka values

K_{a1}=6.9x10^8, K_{a2} = 6.2X10^8, and K_{a3}=4.8X10^{13}

The transformation of H_2PO_4- (aq) to HPO_4^2-(aq)is the second dissociation, so we need to use the Ka2 = 6.2x10-8 in the Henderson-Hasselbalch equation.

Mass of KH2PO4 = 22.0 g , mass of Na2HPO4 = 32.0 g , volume = 1.00 L

First we need to calculate moles of each

Moles of KH2PO4 = 22.0 g / 136.08 g.mol-1

                             = 0.162 moles

Moles of Na2HPO4 = 32.0 g /141.96 g.mol-1

                             = 0.225 moles

[H2PO4-] = 0.162 moles / 1.00 L = 0.162 M

[HPO42-] = 0.225 moles / 1.00 L = 0.225 M

Now we need to calculate the pKa2

pKa2 = -log Ka

       = -log 6.2x10-8

       = 7.21

We know Henderson-Hasselbalch equation

pH = pKa + log [conjugate base] / [acid]

pH = 7.21 + log 0.225 / 0.162

     = 7.35

The pH of a buffer solution obtained by dissolving 22.0 g of KH2PO4 and 32.0 g of Na2HPO4 in water and then diluting to 1.00 L is 7.35

6 0
3 years ago
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