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3 years ago

6

Which ion will correctly complete the formula _________2hpo4?

1 answer:

N76 [4]3 years ago

4 0

The charge of the ion, HPO₄⁻² is equal to -2. This is the same as the one written before it as it appears in the formula of the substance. Since, in the given chemical formula, HPO₄ does not have any multiplier, the charge of the atom or ion that should appear before it is +1. The atoms that will have a charge of +1 are those in group A1. These are Na+, Li+, K+, Rb+, Cs+ and Fr+.

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What are the steps to finding an items density?

Assoli18 [71]

There are 5 steps:
1- measure the mass of the container
2- measure the volume of the liquid
3- measure the combined mass of the liquid and the container.
4-determine the mass of the liquid alone
5-divide the mass by the volume.

3 0

3 years ago

Which of the following is a mixture?

Ne4ueva [31]

It’s water vapor, does this help?

4 0

3 years ago

Consider the equilibrium: HCOOH(aq) + F-(aq) <----> HCOO-(aq) + HF (aq) Given that the Ka of HCOOH = 1.8 x 10-4 and the Ka

Aleks [24]

Hey there!:

K = Ka * Kb / Kw

Ka = 1.8*10⁻⁴

Kb = 10⁻¹⁴ / 6.8*10⁻⁴

K = 1.8*10⁻⁴ * ( 10⁻¹⁴/ 6.8*10⁻⁴ ) * ( 1 / 10⁻¹⁴ )

K = = 1.8 / 6.8

K = 0.265

Answer A

Therefore:

K is less than on the forward reaction is not favorable .

Hope That helps!

8 0

3 years ago

A chemical reaction that is expected to form 325.0 gof product only forms 123.8 g of product. What is the percent yield of this

Tasya [4]

Answer:

$\boxed {\boxed {\sf A. \ 38.1 \%}}$

Explanation:

Percent yield is the ratio of the amount actually produced to how much could theoretically be produced. It is found using this formula:

$\% \ yield = \frac{actual \ yield}{theoretical \ yield} *100$

For this reaction, the theoretical or expected yield is 325.0 grams. The actual yield is 123.8 grams.

$\% \ yield = \frac{ 123.8 \ g }{325.0 \ g }*100$

Divide.

$\% \ yield = 0.380923077 *100$

$\% \ yield = 38.0923077$

Round to the nearest hundredth. The 9 in the hundredth place tells us to round the 0 to a 1 .

$\% \ yield \approx 38.1$

The percent yield is about <u>38.1%</u>

5 0

3 years ago

Read 2 more answers

The temperature of 15.71 grams of gold rises from 32°C to 1,064°C, and then the gold melts completely. If gold’s specific heat i

antoniya [11.8K]

Answer:Total energy gained by 15.71 g is 3090.6471 joules

Explanation:

Given:

Q = heat gained by the 15.71 gram mass of gold

$Q=mc\Delta T +m\Delta H_{fusion}$

$\Delta T=(T_{final}-T_{initial})=(1064^oC-32^oC)=1032^oC$

c = specific heat capacity of gold = 0.1291 $joules/gram^oC$

m = mass of gold =15.71 g

$Q=15.71 g\times 0.1291 joules/gram^oC (1032^oC) +15.71 g\times 63.5 Joules/gram$

Heat gained by gold = $2093.0621 Joules + 997.585 Joules$

=3090.6471 joules

6 0

3 years ago