a. Deionized water b. Buffer solution (acetic acid, sodium acetate mixture) 6. D

Question

a. Deionized water b. Buffer solution (acetic acid, sodium acetate mixture) 6. Describe what you should do if an acid was accidentally spilled on your hands. 7. A 3.00ml aliquot of 0.001 M NaSCN is diluted to 25.0 ml with 0.2 M Fe(NO,), and 0.1 M HNO a. How many moles of SCN are present? b. If all of the SCN is a complexed with Fe' to form FeNCS, what is the molar concentration of FeNCS? 8. What is the correet procedure of diluting a concentrated acid with water? Why? 9? Three parameters affect the absorbance of a sample, which one is the focus of this ex

Explanation / Answer

6.In case of spills:
Acid spills should be neutralized with sodium bicarbonate and then cleaned up with a paper towel or
sponge. Do not use a strong base, such as sodium hydroxide, to neutralize a strong acid like hydrochloric
acid. The sodium bicarbonate will do the job with much less chance of injury. Base spills should be
neutralized with boric acid and then cleaned with a paper towel or sponge. Do not use acetic acid or
sodium bicarbonate to clean a base spill. The sodium bicarbonate will not neutralize the spill, and acetic
acid could react strongly with the base. If you spill an acid or base on your skin, immediately wash well
with water. Strong bases react with the oils in your skin to produce a soapy feeling layer. Rinse until
well after that feeling is gone. Do not attempt to neutralize a spill on your skin. It can potentially make
the injury worse.

8)Remember, you should never add water to acid. This is because the reaction is exothermic, and the solution may splash out. If you add water to acid, it will be acid which splash onto your skin and being concentrated, it is highly corrosive. Hence, you should always add acid to water slowly.

What is the method to make concentrated acid dilute?
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8 ANSWERS
[Saurav Surve]
Saurav Surve, studied at Thakur College of Science and Commerce
Answered Jan 24, 2015 · Upvoted by Chris Marlowe, Bachelors degree in Chemistry from Rutgers University in 19…
Continue Reading
1.   Cool water in an ice bath when using concentrated acids.
This step is only necessary when you'll be handling extremely concentrated acid solutions, such as 18M sulfuric acid, or 12M hydrochloric acid.Cool the water you'll be using by keeping it in a container surrounded by ice for at least 20 minutes before the dilution begin. For most dilutions, the water can be at room temperature.

2.    Add distilled water to a large flask.
For projects involving careful measurement, such as titration, use a volumetric flask. For most practical purposes, an Erlenmeyer flask can be used instead. In either case, choose a container that can easily contain your total desired volume, with plenty of space remaining, to minimize splashes over the rim.

3.   Add a tiny quantity of acid.
If using a small volume of acid, use a graduated (Mohr) pipette or volumetric pipette with a rubber bulb on top. For larger volumes, place a funnel in the neck of the flask, and slowly pour in a small quantity of the acid using a graduated cylinder.


4.    Allow the solution to cool off.
Strong acids may generate lots of heat when added to water. If the acid was highly concentrated, the solution may splatter or produce corrosive fumes. If this happens, you will need to perform the entire dilution in very small doses, or cool the water in an ice bath before you continue.


5.    Add the remaining acid in small doses.
Allow the solution time to cool off between each dose, especially if you notice heat, fumes, or spatter. Continue until the required amount of acid has been added.

6.    Stir the solution.

For best results, you can stir the solution with a glass stirring rod after each addition of acid. If the size of the flask makes this impractical, stir the solution after the dilution is complete and the funnel is removed.



Tips

Always add acid to the water, not the other way around. When the substances meet, they will produce a large amount of heat. The more water is involved, the more of a heat sink you have to absorb this heat, preventing boiling and splattering.
When mixing two acids, always add the stronger acid to the weaker.
It is possible to add half the required amount of water, diluting it fully, then slowly mixing in the remaining water. This is not recommended for concentrated solutions.

Source: wikihow.com
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[Chris Chan]
Chris Chan, Let's party - I'll drop the acid and you shall drop the base!
Answered Nov 3, 2016

Add concentrated acid to water slowly with continuous stirring.

Remember, you should never add water to acid. This is because the reaction is exothermic, and the solution may splash out. If you add water to acid, it will be acid which splash onto your skin and being concentrated, it is highly corrosive. Hence, you should always add acid to water slowly.

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[Muhannad Almemar]
Muhannad Almemar, worked at Bioengineering Master Student
Answered Apr 23, 2016

In order to dilute an acid, first of all you have to decide the concentration of desired (C2) and of course you have to know the concentration of the original acid solution that you wanna dilute (C1). In addition you have to decide the volume of interest of the diluted solution you gonna get (V2).
Make sure that C1 and C2 are given in the same unit for example both of them in molarity (M).
After you get these values you have to use this formula: C1.V1=C2.V2 which means:
solution's concentration x its volume = the diluted solutions' concentration x its volume
Using this formula you can get the value of V1. Now you know how much voulme you need to take from the original solution. In order to know how much water you should add to V1 calculate it by: V2-V1 the result is the amount of water which you have to add to V1.
Read the relevant chemical safety cards online and according to them you can start diluting your acid by adding V1 to the (V2-V1) water carefully.

9)

There are a range of factors that can affect the ultraviolet and visible absorption characteristics of an organic compound. These are attributed to:

solvent
concentration of the sample
pH of the sample
temperature of the sample.

Uncontrolled changes in these factors can introduce inaccuracy and imprecision by altering the position ( [lambda] max) and intensity ( [epsilon] max) of the absorption peaks of the chromophore in the compound. The analyst must control these parameters if comparison of spectra is to be meaningful and if quantitative results are to be valid.

With the job of the analyst in mind, sample and standard preparation will play a key role particularly in regard to using standardised conditions.

Effect of Solvent

The choice of solvent can shift peaks to shorter or longer wavelengths. This will depend on the nature of the interaction of the particular solvent with the environment of the chromophore in the excited state of the molecule.

Depending on the chromophore in the particular analyte, changes in the polarity of the solvent can influence shifts to longer or shorter wavelengths. For instance, it is usually seen that ethanol solutions give longer wavelength maxima than hexane solutions.

Effect of Sample Concentration

As you might expect, sample concentration is proportional to the intensity of the absorption. At high concentrations however, molecular interactions (for example, polymerisation) can take place causing changes to the position and shape of absorption bands. Such an outcome can affect the linearity of the relationship between sample concentration and absorbance (remember Beer’s Law).

Such effects need to be identified and taken into consideration for quantitative work.

Effect of Sample pH

The pH of the sample solution can have a significant impact on absorption spectra. The mechanism for this is primarily a shift in the equilibrium between the different chemical forms of an analyte. To illustrate this, pH indicators used in acid/base titrations change colour at a particular pH because the chemical form of the indicator-compound undergoes a change at this point.

If pH is known to be a factor, a remedy is to prepare the sample in a suitable buffer solution so as to maintain the pH at a steady value. The buffer though needs to be transparent over the wavelength range of the measurements – if the buffer absorbs radiation, absorbance readings attributed to the analyte may be higher than they should because the buffer and analyte absorptions will add together at each wavelength.

Effect of Sample Temperature

Temperature impacts absorption measurements by various means:

Expansion or contraction of the solvent - leading to lower/higher concentrations and absorbances, a particular issue with some organic solvents.
Shifts in equilibria between the chemical forms of an analyte – the nature of the absorbing species may be changed.

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