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EastWind [94]
3 years ago
6

Agitation prevents settling in a?

Chemistry
1 answer:
VashaNatasha [74]3 years ago
5 0
D gaseous mixture I hope it helps
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Directions are in the picture
Mrrafil [7]

Answer:

Question Clear

Explanation:

Make sure your question is clear.

6 0
3 years ago
What is the ph value of the produced solution when hcl reacts with naoh ?
algol13

Answer:

The answer to your question is: 7

Explanation:

The reaction between HCl and NaOH is a neutralization reaction, that means that the products will be water and a salt and the pH will be 7.

                     HCl + NaOH  ⇒  NaCl + H₂O

4 0
3 years ago
What evidence from the experiment shows that conduction occurred? In your answer, be sure to include the materials involved in t
velikii [3]

Answer:

Explanation:

The melting of the chocolate pieces one by one showed that it was caused by heat flowing through the foil bridge. The transfer of heat happened between the foil bridge and the chocolate pieces because they were touching each other.

5 0
3 years ago
Read 2 more answers
Farmers who raise cotton once used arsenic acid, H₃AsO₄, as a defoliant at harvest time. Arsenic acid is a polyprotic acid with
Stels [109]

Explanation:

The reaction equation will be as follows.

      H_{3}AsO_{4} \rightleftharpoons H_{2}AsO^{-}_{4} + H^{+}

Hence, the expression for K_{a} is as follows.

            K_{a} = \frac{[H_{2}SO^{-}_{4}][H^{+}]}{[H_{3}AsO_{4}]}

Let us assume that the concentration of both [H_{2}AsO^{-}_{4}] and [H^{+}] is x.

           2.5 \times 10^{-4} = \frac{x \times x}{0.5}

                          x = 0.01118034

This means that the concentration of [H^{+}] is 0.01118034.

Since, we know that the relation between pH and concentration of hydrogen ions is as follows.

              pH = -log [H^{+}]

                    = -log (0.01118034)

                    = 1.958

Thus, we can conclude that the pH of a 0.500 M solution of arsenic acid is 1.958.

6 0
3 years ago
In Part A, you found the amount of product (1.80 mol P2O5 ) formed from the given amount of phosphorus and excess oxygen. In Par
Finger [1]

First step is to balance the reaction equation. Hence we get P4 + 5 O2 => 2 P2O5

Second, we calculate the amounts we start with

P4: 112 g = 112 g/ 124 g/mol – 0.903 mol

O2: 112 g = 112 g / 32 g/mol = 3.5 mol

Lastly, we calculate the amount of P2O5 produced.

2.5 mol of O2 will react with 0.7 mol of P2O5 to produce 1.4 mol of P2O5.

This is 1.4 * (31*2 + 16*5) = 198.8 g

3 0
3 years ago
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