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Bi2(CO3)3 Name of this compound

Keith_Richards [23]

Answer:

The name of this compound is :

Bi2(CO3)3 = Bismuth Carbonate

Explanation:

The name of the compound is derived from the name of the elements present in it.

The rule followed while naming the compound are:

1. The first element (always the cation) is named as such .

2. The second element (The anion) end with "-ate , -ide ," etc

3. NO prefix is added while naming the first element.

For example : Bi2 can't be named as Dibismuth

Na2 = Can't be named as disodium

Hence the compound :

Bi2(CO3)3 contain two element : Bi and CO3. Here , Bi = cation (named as such) and CO3 = anion (named according to rules)

Bi = Bismuth

CO3 = carbonate

Bi2(CO3)3 = Bismuth Carbonate

The molecular mass of this compound is :

Molecular mass = 2 (mass of Bi) + 3(mass of C) + 6(mass of O)

= 2 (208.98)+3(12.01)+6(15.99)

= 597.987 u

5 0

2 years ago

How many particles are present in 10.0 moles of table salt?

Dima020 [189]

1.01 x 10^24 molecules.

Explanation:

To calculate the number of molecules in a given number of mole, we can simply multiply by Avogadro's number which is equal to 6.022 x 10 ^23.

Therefore,

10 molecules = 1.68 mol x (6.022 x 10^23 molecules) / (1 mol = 1.01 x 10^24) molecules.

I hope this helps :)

7 0

2 years ago

An analytical chemist is titrating of a solution of ethylamine with a solution of . The of ethylamine is . Calculate the pH of t

Elenna [48]

Answer:

pH=11.

Explanation:

Hello!

In this case, since the data is not given, it is possible to use a similar problem like:

"An analytical chemist is titrating 185.0 mL of a 0.7500 M solution of ethylamine(C2HNH2) with a 0.4800 M solution of HNO3.ThepK,of ethylamine is 3.19. Calculate the pH of the base solution after the chemist has added 114.4 mL of the HNO3 solution to it"

Thus, for the reaction:

$C_2H_5NH_2+H^+\rightleftharpoons C_2H_5NH_4^+$

Tt is possible to compute the remaining moles of ethylamine via the following subtraction:

$n_{ethylamine}=0.1850L*0.7500mol/L=0.1365mol\\\\n_{acid}=0.1144L*0.4800mol/L=0.0549mol\\\\n_{ethylamine}^{remaining}=0.1365mol-0.0549mol=0.0816mol$

Thus, the concentration of ethylamine in solution is:

$[ethylamine]=\frac{0.0816mol}{0.1850L+0.1144L}=0.2725M$

Now, we can also infer that some salt is formed, and has the following concentration:

$[salt]=\frac{0.0549mol}{0.1850L+0.1144L}=0.1834M$

Therefore, we can use the Henderson-Hasselbach equation to compute the resulting pOH first:

$pOH=pKb+log(\frac{[salt]}{[base]} )\\\\pOH=3.19+log(\frac{0.1834M}{0.2725M})\\\\pOH=3.0$

Finally, the pH turns out to be:

$pH=14-pOH=14-3\\\\pH=11$

NOTE: keep in mind that if you have different values, you can just change them and follow the very same process here.

Best regards!

4 0

2 years ago

Can you pls tell me advantages and disadvantages of chemistry in specific

katrin2010 [14]

Advantages

Chemistry helps you to understand the world around you.

Basic knowledge of chemistry helps you to read and understand product labels.

Chemistry can help you make informed decisions.

Chemistry is at the heart of cooking.

A command of chemistry can help keep you safe!

Disadvantages 

It isn't a sustainable form of energy.

It can be expensive.

Some forms of chemical energy are quite rare.

It can produce harmful waste.

It can be used to create devastating weapons.

It offers short-term benefits for long-term consequences.

6 0

2 years ago

The density of an aqueous solution containing 10.0 percent of ethanol (C2H5OH) by mass is 0.984 g/mL. (a) Calculate the molality

Mrrafil [7]

Answer:

a. 2.41 molal

b. 0.21 M

c. 58.5 mL

Explanation:

First of all let's think the data 10 % by mass, which means, that 10 grams from the solute is contained in 100 g of this solution.

So If we know solution density, we can get its volume.

Solution density = Solution mass / Solution volume

0.984 g/ml = 100 g / Solution volume

Solution volume = 100 g/ 0.984g/ml

Volume = 101.6 mL

As we have 10 g of solute, 100 g of solution, we have 90 g of solvent.

Solute mass + Solvent mass = Solution mass

How many moles do we have in 10 g of ethanol?

Molar mass of ethanol: 46.07 g/m

Mass / molar mass = Moles

10 g/ 46.07 g/m = 0.217 mol

This quantity is in 90 g of solvent and 101.6 mL of solution. For molality and molarity, we should use a rule of three to find out the moles in 1 kg of solvent and 1 L of solution.

1 L = 1000 mL

1kg = 1000 g

Molality

90 g _____ 0.217 moles

1000 g _____ (1000 . 0.217)/ 10 = 2.41 molal

Molarity

101.6 mL ___ 0.217 moles

1000 mL ____ (1000 . 0.217) / 101.6 = 0.21 M

What volume of the solution would contain 0.125 mole of ethanol?. Let's think a new rule of three.

0.217 moles of solute ___ are in __ 101.6 mL of solution

0.125 moles of solute___ are in (0.125 . 101.6)/0.217 = 58.5 mL

6 0

2 years ago