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2 years ago

2KI(aq) + Pb(NO,)(aq) › PbI(s) + 2KNOg(aq) Balance the equation

Chemistry

1 answer:

azamat2 years ago

5 0

Answer:

Explanation:

There are some mistakes in writing the equation. However, Please check the below one and contact me again if necessary.

2KI(aq) + Pb(NO₃)₂ (aq) -> PbI₂ (s) + 2KNO₃

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Care needs to be taken when adding acid to base because

nikitadnepr [17]

<span>Mixing an acid and a base results in neutralization, but the results are potentially dangerous. No matter which acid or base is used, the resulting solution is water and varying types of salt. The process of neutralization often involves the substances heating up when they come together. If the solution heats up too much or too fast, a violent explosion or the creation of harmful or flammable gases is a possibility. This occurs when the chemicals are mixed too quickly, the acid and base are too strong or if there is no available salt to be made in the solution.</span>

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2 years ago

When preparing a buret for use in lab, the buret must always be cleaned thoroughly. prior to being filled with solution, the bur

erastova [34]

It is rinsed one last time with the solution to be measured because if there is water in the burret, then it could alter the results. Slightly, but it is still altering it.

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3 years ago

2. Classify the following solutions as acidic, basic, or neutral at 25OC.

PilotLPTM [1.2K]

Answer: a) pH = 13.00 : basic

b) $[H_3O^+]=1.0\times 10^{-12}$ : basic

c) pOH = 5.00 : basic

d) $[OH^-]=1.0\times 10^{-9}$ : acidic

Explanation:

pH or pOH is the measure of acidity or alkalinity of a solution.

pH is calculated by taking negative logarithm of hydrogen ion concentration.

$pH=-\log [H_3O^+]$

Acids have pH ranging from 1 to 6.9 and bases have pH ranging from 7.1 to 14.Neutral substances have pH of 7.

a) pH = 13.00

As pH is more than 7, the solution is basic.

b) $[H_3O^+]=1.0\times 10^{-12}$

Putting in the values:

$pH=-\log[1.0\times 10^{-12}]$

$pH=12$

As pH is more than 7, the solution is basic.

c) pOH = 5.00

$pH+pOH=14.0$

$pH=14.0-5.00=9.00$

As pH is more than 7, the solution is basic.

d) $[OH^-]=1.0\times 10^{-9}$

Putting in the values:

$pOH=-\log[1.0\times 10^{-9}]$

$pOH=9.00$

$pH+pOH=14.0$

$pH=14.0-9.00=5.00$

As pH is less than 7, the solution is acidic.

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3 years ago

Select all correct answers.

Jlenok [28]

Answer: It showed that all atoms contain electrons.

Explanation:

J.J. Thomson's experiments inside a cathode ray tube in the presence of an electric field showed that all atoms contain tiny negatively charged subatomic particles "electrons".

Also, Thomson's plum pudding model of the atom had negatively-charged electrons embedded within a positively-charged "soup."

Furthermore, Rutherford's gold foil experiment showed that the atom is mostly empty space with a tiny positively-charged nucleus.

Then, Rutherford proposed the nuclear model of the atom based on these results.

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3 years ago

The temperature of a 95.4 g piece of Cu increases from 25.0 °C to 48.0 °C when the Cu absorbs 849 J of heat. What is the specifc

melisa1 [442]

<h3>Answer:</h3>

0.387 J/g°C

<h3>Explanation:</h3>

To calculate the amount of heat absorbed or released by a substance we need to know its mass, change in temperature and its specific heat capacity.
Then to get quantity of heat absorbed or lost we multiply mass by specific heat capacity and change in temperature.
That is, Q = mcΔT

in our question we are given;

Mass of copper, m as 95.4 g

Initial temperature = 25 °C

Final temperature = 48 °C

Thus, change in temperature, ΔT = 23°C

Quantity of heat absorbed, Q as 849 J

We are required to calculate the specific heat capacity of copper

Rearranging the formula we get

c = Q ÷ mΔT

Therefore,

Specific heat capacity, c = 849 J ÷ (95.4 g × 23°C)

= 0.3869 J/g°C

= 0.387 J/g°C

Therefore, the specific heat capacity of copper is 0.387 J/g°C

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2 years ago