Determining The Molarity Of An Acidic Solution

2. To titrate a hydrochloric acid solution of “known” concentration with standardized 0.5M sodium hydroxide.

H. How would you prepare 10 mL of a 0.25M HCl solution if 1M HCl was available? How much

The concentration or molarity of a solution can be seen through the ratio of solute amount to solution volume. This means that when you take the solute amount of a solution in moles and divide it by its volumes in liters you are able to find the solution’s overall concentration or molarity. This is proven in my data table below labeled, Molarity Simulation Data, and it helps to show that when you get the moles of a solute and the volume of the solvent you can easily and accurately figure out the molarity of the solution you are investigating. For example, when there were .75 moles of an energy drink power, and only .25 liters of water to mix it in, as shown in #3 of my data table, I was able to identify the molarity as 3 M through the process of division The way I executed this experiment lets me to see the impressionable relationship between the solute amount in moles and the solution volume in liters and how they affect molarity of a solution. The data table allows me to demonstrate this pattern. My argument is, the molarity of an aqueous solution can be found if you take the moles found in a given solute and divide them by the volume of the solvent. The data presented in this paper proves that the given formula shows the dependent, mathematical relationship that all three of these factors

EXPERIMENT 3. ACID-BASE TITRATIONS: DETERMINATION OF CARBONATE BY TITRATION WITH HYDROCHLORIC ACID BACKGROUND Carbonate Equilibria In this experiment a solution of hydrochloric acid is prepared, standardized against pure sodium carbonate, and used to determine the percentage of carbonate in a sample. An aqueous solution of hydrochloric acid is almost completely dissociated into hydrated protons and chloride ions. Therefore, in a titration with hydrochloric acid the active titrant species is the hydrated proton. This species is often written H3O+, although the actual form in solution is more correctly (H2O)nH+. For convenience we designate it simply H+. Carbonate in aqueous solution acts as a base; that is, it is able to accept a

The results showed the molarity of the NaOH solution. This experiment was completed twice and a new average molarity

9. How many moles of NaOH would be needed to completely react with all of the excess HCl determined in problem 8?

ii. The second part of the titration series involves titration of NaOH with Hydrochloric acid (HCL). Again, three reps of titration and a blank titration have to be completed. A volumetric pipet is used to measure 10.00mL of HCL into three labeled conical flasks. Then the flasks are filled with deionized water until about the 50mL mark. A buret is

5. Use a 50mL or 100mL graduated cylinder to measure approximately 50mL of hydrochloric acid.

The colour change because of addition of base that remove hydrogen and produce more phenolphthalein ions. (Reference.com, 2016). The average volume of NaOH is 77.1 mL when the colour of the solution had changed into faint pink (Revised Spring NF, p.4, 2004). In 2.1.4, Pearson square method was used for dilution. This method used arithmetic ratio technique known as allegation. Allegation is “a process or rule for the solution of problems concerning the compounding or mixing of ingredients differing in price or quality” (small & us, 2016). Pearson square method is a simple method that used when combine two elements together with simple ratios and produce higher value (Wagner and Stanton, 2012). Formula M1V1=M2V2 also can be used in this problem if B=0 which is B is molarity of dilute solution but if B≠0, Pearson square method must be used. Lastly, the volume HCL needed is 1.9 mL and molarity of HCL gain is 0.01

In addition to this, my group found calibration error of our pH meter in the experiment 1.2. It is possible that our pH meter was not very accurate from the beginning of our experiment. Answers to post-lab questions: The theoretical pH of the acetate buffer before adding acid or base was about 4.5, and actual value of pH was 5.0.

Using the equation of the reaction for the HCl titration and the calculation from your practical books; calculate the exact concentration of the sodium hydroxide used. Show your calculation

mL HCl titrated * 1L/1000 mL * mol. Of standardized HCl/1L * 1/.10L sample * 1000mmol/1 mol = mmol HCl/L

500 mL of .01 M HCl solution was prepared first be cleaning a 500 mL volumetric flask by swirling with distilled water. Then, 200 mL of

Acid-base titrations are a commonly used laboratory practice, used to determine the concentration of a particular acid or a particular base by neutralizing them with a known concentration of another acid or base. Acid-base titrations are tracked and measured with the use of an indicator, which causes a color change whenever the pH changes between specific values. An indicator is composed of an acid or base whose conjugate acid or conjugate base has a color different from that of the original compound.1 The use of the indicator allows us to observe and note the neutralization of a titration which occurs at the end point. Hydrochloric acid (strong acid) and sodium hydroxide (strong base), are the most commonly used acid and base in experiments. A strong acid dissociates (or ionizes) completely in aqueous solution to form hydronium ions (H3O+), while a strong base dissociates completely in aqueous solution to form hydroxide ions (OH-).1 In this experiment we used potassium hydrogen phthalate and sodium carbonate as primary standards. These two are compounds used as primary standards, which are tools that aid in determining the exact concentration of acids and bases due to their characteristics (See Discussion).

Acids - Compounds that have properties with the kinds of reactions they undergo. Acids also release or donate hydrogen ions. This relates to our lab because orange juice is filled with citric acid, and we are testing the amount of acid (pH)