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Airida [17]
3 years ago
13

Which compounds yield hydrogen ions as the only positive ions in an aqueous solution?

Chemistry
2 answers:
noname [10]3 years ago
7 0
The answer is (1) because both are acids.
stich3 [128]3 years ago
4 0
I believe the answer would be <span>(1) H2CO3 and HC2H3O2. Hope I helped! :)</span>
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How many grams are there in 1.18 X 1026 atoms of iridium?
stealth61 [152]
You want to divide by avagadros number (6.22 x 10^23). This will cancel the atoms unit and give moles, moles of Iridium. Now you want to calculate the atomic mass of Iridium which is in units of grams per mole. Multiply these two numbers and the moles will cancel giving you grams.

Setting up a dimension analysis type of thing helps tremendously. See what you have to cancel in order to get what you want. We canceled the atoms, then we canceled the moles, and then we got grams.
4 0
3 years ago
Given the following reaction: 3CuCl2(aq) 2Na3PO4(aq) --&gt; Cu3(PO4)2(s) 6NaCl(aq) MM (g/mol) 134.45 163.94 380.58 58.44 If 285
nata0808 [166]

Answer:

227.78g of the precipitate are produced

Explanation:

Based on the reaction, 3 moles of CuCl2 produce 1 mole of Cu3(PO4)2 (The precipitate).

To solve this question we need to find the moles of CuCl2 added. With these moles and the reactio we can find the moles of Cu3(PO4)2 and its mass as follows:

<em>Moles CuCl2:</em>

285mL = 0.285L * (6.3mol / L) = 1.7955 moles CuCl2

<em>Moles Cu3(PO4)2:</em>

1.7955 moles CuCl2 * (1mol Cu3(PO4)2 / 3mol CuCl2) = 0.5985 moles Cu3(PO4)2

<em>Mass Cu3(PO4)2 -380.58g/mol-</em>

0.5985 moles Cu3(PO4)2 * (380.58g/mol) =

227.78g of the precipitate are produced

7 0
3 years ago
How many grams are in 6.50 moles of h2so4?
GREYUIT [131]
You multiply 6.50 by the molar mass of H2SO4. 
7 0
3 years ago
Read 2 more answers
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Kisachek [45]

Answer:

yes the ones u chose are correct.

Explanation:

8 0
3 years ago
Iday!' Read the following phrases from the article. 1. Full-scale war 2. Braces for a full invasion 3. Hostile act 4. Defenses o
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Answer:

c.

Explanation:

7 0
2 years ago
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