CHEMISTRY COLLEGE

Systematic name for: Silver Nitrate.molar mass of Ag:
molar mass of N:
molar mass of O:

and the overall molar mass for Silver Nitrate.

Answers

Answer 1

Answer:

Answer:

$AgNO_3$ ,Molar mass =169.87 g/mol

Explanation:

The systematic name for silver nitrate is $AgNO_3$

Now we have to calculate the molar mass of $AgNO_3$

Molar mass of Ag = 107.87 g/mol

Molar mass of N =14 g/mol

Molar mass of O =16 g/mol

So the molar mass of silver nitrate ( $AgNO_3$ ) is

$=(1* 107.87+1* 14+3* 16)=169.87g/mol$

Related Questions

Consider two aqueous solutions of NaCl. Solution 1 is 4.00 M and solution 2 is 0.10 M. In what ratio (solution 1 to solution 2) must these solutions be mixed in order to produce a 0.86 M solution of NaCl
A 9.70-g piece of solid CO 2 is allowed to sublime in a balloon. The final volume of the balloon is 1.00 L at 298 K. What is the pressure of the gas inside the balloon?a. 5.39 atmb. 2.37  102 atmc. 2.52 atmd. 0.186 atme. none of these
Identify which of the following equations are balanced.A. 6Li(s)+N2(g)→2Li3N(s)6Li(s)+N2(g)→2Li3N(s).B. 2KMnO4(s)→K2MnO4(s)+MnO2(s)+O2(g). C. 2KClO3(s)→2KCl(s)+O2(g)2KClO3(s)→2KCl(s)+O2(g). D. Mg(s)+N2(g)→Mg3N2(s)Mg(s)+N2(g)→Mg3N2(s).
MEASUREMENT AND MATTER Interconverting temperatures in Celsius and Kelvins The metal osmium becomes superconducting at temperatures below 655.mk Calculate the temperature at which osmium becomes superconducting in degrees Celsius. Be sure your answer has the correct number of significant digits. Ac
If the mass percentage composition of a compound is 72.1% Mn and 27.9% O, its empirical formula is

A student obtained the following data for the rearrangement of cyclopropane to propene at 500 °C. (CH2)3(g)CH3CH=CH2(g) [(CH2)3], M 0.128 6.40×10-2 3.20×10-2 1.60×10-2 time, min 0 14.4 28.8 43.2 (1) What is the half-life for the reaction starting at t=0 min? min What is the half-life for the reaction starting at t=14.4 min? min Does the half-life increase, decrease or remain constant as the reaction proceeds? _________ (2) Is the reaction zero, first, or second order? _______ (3) Based on these data, what is the rate constant for the reaction? min-1

Answers

Explanation:

CH2)3(g)CH3CH=CH2(g) [(CH2)3], M time, min

0.128 0

6.40×10-2 14.4

3.20×10-2 28.8

1.60×10-2 43.2

(1) What is the half-life for the reaction starting at t=0 min? min

Half life is the amount of time required for a substance to decay by half of it's initial concentration.

Starting form 0, the initial concentration = 0.128

After 14.4 mins, the final concentration is now exactly half of the initial concentration. This means 14.4 min is the half life starting from t=0min

What is the half-life for the reaction starting at t=14.4 min?

Starting form 14.4min, the initial concentration = 6.40×10-2

After 14.4 mins (28.8 - 14.4), the final concentration is now exactly half of the initial concentration. This means 14.4 min is the half life starting from t=14.4min

Does the half-life increase, decrease or remain constant as the reaction proceeds?

The half life is a constant factor, hence it remains constant as the reaction proceeds.

(2) Is the reaction zero, first, or second order?

Because the half life is independent of the concentration, it is a first order reaction.

In a zero order reaction, the half life Decreases as the reaction progresses; as concentration decreases.

In a first order reaction, the half life Increases with decreasing concentration.

(3) Based on these data, what is the rate constant for the reaction? min-1

The realtionship between the half life and rate onstant is;

k = 0.693 / half life

k = 0.693 / 14.4

k = 0.048125 min-1

2. Which test for iron(II) ions is conclusive

Answers

The conclusive test for iron(II) ions is the test by the use of potassium hexacyanoferrate III solution.

In qualitative analysis certain reagents are used to test for the presence of certain cations or anions. Those reagents react in a certain way with those reagents. Usually, a positive test may involve a color change, formation of a precipitate or evolution of a gas.

In the case of iron(II) ions, potassium hexacyanoferrate III solution is used in the conclusive qualitative test for the ion. A positive test involves the appearance of a deep blue precipitate.

Learn more: brainly.com/question/6955504

Answer:

please brainlist answer

Explanation:

The addition of K 3 Fe(CN) 6 to a solution causes the formation of a deep blue precipitate which indicates that iron(II) ions are present.

A buffer solution is 0.413 M in HF and 0.237 M in KF. If Ka for HF is 7.2×10-4, what is the pH of this buffer solution?

Answers

Answer:

2.90

Explanation:

Any buffer system can be described with the reaction:

$HA~->~H^+~+~A^-$

Where $HA$ is the acid and $A^-$ is the base. Additionally, the calculation of the pH of any buffer system can be made with the Henderson-Hasselbach equation:

$pH=pKa~+~Log([A^-])/([HA])$

With all this in mind, we can write the reaction for our buffer system:

$HF~->~H^+~+~F^-$

In this case, the acid is $HF$ with a concentration of 0.413 M and the base is $F^-$ with a concentration of 0.237 M. We can calculate the pKa value if we do the "-Log Ka", so:

$pKa~=~-Log(7.2X10^-^4)=~3.14$

Now, we can plug the values into the Henderson-Hasselbach

$pH=~3.14~+~Log(([0.237~M])/([0.413~M]))~=~2.90$

The pH value would be 2.90

I hope it helps!

After clamping a barrette to a ring stand you noticed that the set up is tippy and unstable what should you do to stabilize the set up?

Answers

Move the buret clamp to a ring stand with a larger base.

HELP ME PLEASE I will mark brainliest

Answers

Answer:

Nice pic there

Explanation:

No need

Chlorine (Cl2Cl2) is a strong germicide used to disinfect drinking water and to kill microbes in swimming pools. If the product is Cl−Cl−, was the elemental chlorine oxidized or reduced?