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3 years ago

What are the reagents for BaCO3(s)

Chemistry

1 answer:

Wittaler [7]3 years ago

6 0

The reagents for BaCO₃ is

BaO and CO₂

Explanation

Reagent is a substance that bring about a chemical reaction when added to a system.

Some reagent may be added to see if a reaction has occurred.

BaO and Co₂ are reagent since they react to produce BaCO₃ as below

BaO(s) + CO₂(g) → BaCO3(s)

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What are the different chemical properties of the element Cobalt?

larisa [96]

Answer:

It is a hard ferromagnetic, silver-white, lustrous, brittle element.

It is stable in air and does not react with water.

Like other metals, it can also be magnetized.

With dilute acids, it reacts slowly.

The metal melts at 1495 °C and boils at 2927 °C

Explanation:

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3 years ago

How is the atmosphere like an ocean

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3 years ago

Read 2 more answers

How would the pH value of an aqueous solution change, when the hydronium ion concentration is increased by a factor of 10?

Anna71 [15]

Answer:

Increasing H⁺ by 10x => pH decreases by 1 unit

Explanation:

In general, adding H⁺ ions to any aqueous solution ALWAYS causes pH values to fall ( decrease ). Just as adding OH⁻ ions to an aqueous solution causes pH values to rise ( increase ).

Here's a simple calculation demonstrating this...

Given 0.01M HCl(aq) => 0.01M H⁺(aq) + Cl⁻(aq) => pH = -log(0.01) = 2.00

Increase [H⁺] by 10x => 0.10M H⁺(aq) => pH = -log[H⁺] = -log(0.10) = 1.00

Solution with higher H⁺ concentration shows pH decreasing by 1 unit.

______________________________________________________-

Just to support the above statement about adding OH⁻ ions showing an increase in pH values, the following is also provided FYI ..

Given 0.01M NaOH(aq) => 0.01M OH⁻(aq) + Na⁺(aq) => pOH = -log(0.01) = 2.00 => pH = 14 - pOH = 14 - 2 = 12

Increase [OH⁻] by 10x => 0.10M OH⁻(aq) => pOH = -log[OH⁻] = -log(0.10) = 1.00 => pH = 14 - pOH = 14 - 1 = 13

Increasing [OH⁻] by 10x => increasing pH by 1 unit.

Solution with higher H⁺ concentration shows pH decreasing by 1 unit.

______________________________________________________

Remember, for any aqueous solution ...

=> Adding H⁺ => always decreases pH

=> Adding OH⁻ => always increases pH

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3 years ago

Use the drop-down menus to identify the effect of each mutation.

krek1111 [17]

Answer:

1 neutral

2 beneficial

3 harmful

Explanation:

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4 years ago

Read 2 more answers

PH is a logarithmic scale used to indicate the hydrogen ion concentration, [H+], of a solution: pH=−log[H+] Due to the autoioniz

ruslelena [56]

Answer:

A) pH = 2.42
B) pH = 12.00

Explanation:

The dissolution of HCl is HCl → H⁺ + Cl⁻

To solve part A) we need to calculate the concentration of H⁺, to do that we need the moles of H⁺ and the volume.

The problem gives us V=2.5 L, and the moles can be calculated using the molecular weight of HCl, 36.46 g/mol:

$0.35g_{HCl}*\frac{1mol_{HCl}}{36.46g_{HCl}} *\frac{1molH^{+}}{1mol HCl}$ = 9.60*10⁻³ mol H⁺

So the concentration of H⁺ is

[H⁺] = 9.60*10⁻³ mol / 2.5 L = 3.84 * 10⁻³ M

pH = -log [H⁺] = -log (3.84 * 10⁻³) = 2.42

The dissolution of NaOH is NaOH → Na⁺ + OH⁻
Now we calculate [OH⁻], we already know that V = 2.0 L, and a similar process is used to calculate the moles of OH⁻, keeping in mind the molecular weight of NaOH, 40 g/mol:

$0.80g_{NaOH}*\frac{1mol_{NaOH}}{40g_{NaOH}} *\frac{1molOH^{-}}{1mol NaOH}$ = 0.02 mol OH⁻

[OH⁻] = 0.02 mol / 2.0 L = 0.01

pOH = -log [OH⁻] = -log (0.01) = 2.00

With the pOH, we can calculate the pH:

pH + pOH = 14.00

pH + 2.00 = 14.00

pH = 12.00

5 0

3 years ago