What would be the MOLARITY (M) of the NaBr in the same buffer solution, if its concentration is now 0.9% (w/v)?

1 answer:

6 0

If by buffer solution you mean, a solution of the same concentration, the molarity (M) would stay the same. You would just have a greater volume.

You might be interested in

Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming of natural

hoa [83]

Answer: The net chemical equation is given below.

Explanation:

To determine the net chemical equation, we will look into the intermediate steps:

Step 1: Formation of ammonia from hydrogen and nitrogen gas.

$N_2(g)+3H_2(g)\rightarrow 2NH_3(g)$ ......(1)

Step 2: Formation of nitric acid from ammonia and oxygen gas.

$NH_3(g)+2O_2(g)\rightarrow HNO_3(g)+H_2O(g)$ .....(2)

The net chemical equation for the formation of nitric acid from hydrogen gas, nitrogen gas and oxygen gas follows by adding both the equations, we get:

$N_2(g)+2O_2(g)+3H_2(g)\rightarrow HNO_3(g)+H_2O(g)+NH_3(g)$

By Stoichiometry of the reaction:

1 mole of hydrogen gas reacts with 2 moles of oxygen gas and 3 moles of hydrogen gas to produce 1 mole of nitric acid, 1 mole of water and 1 mole of ammonia.

Hence, the net chemical equation is given below.

4 0

3 years ago

A first-order reaction has a half-life of 20.0 minutes. Starting with 1.00 × 1020 molecules of reactant at time t = 0, how many

zalisa [80]

Half-life time of a reaction is time at which reactant concentration becomes half of its initial value.

Half-life of the first order reaction is 20 min. Rate constant can be calculated as follows:

$K=\frac{0.6932}{t_{1/2}}=\frac{0.6932}{20 min}=0.03466 min^{-1}$