Titration Definition and 278 Threads

Consider the titration of the weak base analyte methylamine (##\mathrm{CH_3NH_2}##) with the strong acid ##\mathrm{HCl}##. Methylamine has a basicity constant of ##K_b=5.6\times 10^{-4}##. We start with a 75mL sample of 0.500M solution of methylamine in water. We titrate with a 0.205 solution...

Suppose we want to find the pH at the equivalence point. The way I know how to do it is the following. Acetic acid has a dynamic equilibrium with water in aqueous solution given by $$\mathrm{CH_3COOH(aq)+H_2O(l)\rightleftharpoons CH_3COO_2^-(aq)+H_3O^+(aq)}\tag{1}$$ We are given...

I tried to solve the problem (problem 1 on this problem set) by noting that titrating to the equivalence point means neutralizing all of the NaOH with the titrant HCl. Since 15.4mL of HCl at 1.0M was used, then 0.00154 mol of HCl was used to neutralize the same amount of NaOH. Therefore, in...

The reason is that at the stoichiometric point the entirety of the analyte has been neutralized and the solution contains only the salt from the neutralization plus the ions from water autoprotolysis. The salt comes from the conjugate acid of the strong base and the conjugate base of the strong...

We start with 25ml of a 0.100M solution of ##\mathrm{HCOOH(aq)}## and as titrant we use a 0.150M solution of ##\mathrm{NaOH(aq)}##. For reference, we can calculate the initial pH of the formic acid solution, which comes out to 2.37. I will go over just the results of the initial calculations...

Here is an example Let me go through the concepts here. The stoichiometric point occurs when the number of moles of acid and base have the same ratio as present in the chemical equation. In the equation shown above, this is a 1:1 relationship. Acetic acid is a weak acid and at the...

Heyy I just started year 12 this year, and my school has already started our IA2 student experiment, I was wondering which experiment would be the best choice for me to do and would help me to achieve a 20/20. 1. Titration experiment 2. Galvanic cell experiment could you also provide a list of...

We used 14ml of a KMNO4 solution of 0.01 Normality, to find the Normality of a (COONa)2 solution. If we took 10ml of the (COONa)2 solution, what should its Normality be? I thought about using the following equation: N1V1=N2V2 Does the stoichiometry of the redox reaction affect the equation...

This question is asking about finding the indicator. I think phenolphthalein will be used as there is a reaction between strong acid and strong base. Is this approach to the question correct? Or am I missing any important concept? Kindly tell

Help! I am confused with my assignment. it was about complex acid base titration. the analyte was citric acid and the titrant was a base. To find it, I need to search for C1V1=C2V2, however during the balanced equation, there is 3 mol of my base that will be reacting to 1 acid. Will the ratio of...

There is 0.019243 mol of CaCO3, and therefore 0.038485 mol of HCL. There is 0011505 mol of HCl in excess after reacting it with CaCO3. The concentration of HCl after water is added is 0.11515 mol/dm3. There is 0.0011515 mol of HCl in 10 cm3 of the new solution, and the same number of moles of...

Use the equivalence volume from the pH curve to calculate the concentration of the acid, HA. I'm not sure which equation to use or how to approach this question (Attached). Please elaborate on the steps on how to answer the question. Thank you!

I got a answer by equation the moles i took the n factor of oxalic acid as 2 and the naoh solution came out to be 2M but i got an answer of 4grams but the answer given is 2 grams am i correct ??

1/ iodine stock solution: mixed 2,5424 g I2 and 24,1525 g KI and made up to 100 ml with water 2/ 150 mg active carbon is mixed with 12,5 ml jodine solution from point 1 / 3/ At equilibrium were performed filtration and titration with 10 ml of the filtrate with a volumetric solution Na2S2O3...

Homework Statement Homework EquationsThe Attempt at a Solution I don’t have a clue on how to do the calculations. I know the equivalency point is at the steepest part of the derivative graph. Please don’t say just figure it out, I truly need help. I haven’t learned titrations in lecture yet...

Homework Statement calculate the number of moles of potassium manganate required to neutralise oxalic acid. 2KMn)4- + 5H2C2O42-+ 16H+ --> 2Mn2+ + 10CO2 + H2O Homework Equations n = c x V n= m/Ar The Attempt at a Solution Moles of oxalic acid = 5x10-4 Volumeol of KMnO4 = 0.01085dm-3...

Cl2(g) + 2I–(aq) -->I2(aq) + 2Cl–(aq) (reaction 1) [2S2O3^(2-)(aq) + I2(aq) --> S4O6(2-)(aq) + 2I–(aq) (reaction 2) Why isn't n(I2)(reaction 2)=2n(S2O3^(2-))(reaction 2). I don't see why this is wrong. <edit: remove size and italics>

Homework Statement 20 ml of decinormal HCl soln. is added to 10 ml decinormal AgNO3 soln. AgCl is precipitated out and excess of acid was back titrated against a decinormal NaOH soln., What volume of NaOH was required for the back titration? 2. The attempt at a solution 10 ml HCl reacts with...

Homework Statement The ratio of KMnO4 to I2 is given by 2 MnO4 - + 16 H+ + 10 I - ⇌ 2 Mn2+ + 5 I2 + 8 H2O the ratio is 2:5 - The ratio of I2 to S2O3 2- is given by 1 I2 + 2 S2O32- ⇌ 2 I-+ S4O5 2- the ratio is 1:2 therefore n(S2O3 2- ) = n(MnO4 - ) x 5 Homework Equations Why the mole of...

Homework Statement 1) for a given reaction to consume one reactant completely, must the equivalents of both reactants be same? for example, I know in the reaction of HCl + NaOH - the equivalents of HCl=equivalents of NaOH for a titration, is it the same for Na2CO3 + HCl? 2) the following is an...

Homework Statement We had a titration lab where we took 1.0 g of NaOH and added it to 50 mL of water. We then took that solution and added 10 mL of it to 500 mL of water, producing a 510 mL solution in total (this became the titrant). We then took 0.4 g of potassium hydrogen phthalate and...

I tried looking for my unknown (209.70 g/mol) online and couldn't find it. The closest I found were H4O7V2(217.907 g/mol) and HCl2I(198.819 g/mol), but I know I am correct to a 2.7% accuracy. What other lists can I use to solve this?

I am confused on a titration question. I understand most of it but I do not see why they do not multiply their answer by 10 at the end because it says 100 cm^3 of water was analysed but that formula gives answers in moles/L so to make it into a liter they should multiply by 10 but they do not ?

Homework Statement Joshua has been gold panning and extracts a mixture of silicate stone and shiny gold-like particles. However Nkosi says these are Fool's Gold i.e Chalcopyrities (Cu Fe S2). They decide to find out how much iron is in the sample by: -Grinding a 30.00g sample to a fine powder...

I am currently performing a school experiment in which I am testing when citric acid decays. We are juicing lemons, filtering them to get a higher concentration of citric acid, placing them in water baths from 10 to 90 degrees Celsius and then titrating them against one mole of sodium hydroxide...

A solution of (NH4)2SO4·FeSO4·6H2O (hydrated ammonium iron(II) sulfate), used as a primary standard, was prepared by dissolving 8.82 g of the crystals in dilute sulfuric acid and making the solution up to exactly 250 cm3 with deionised water. This standard solution was titrated in 25.0 cm3...

Really struggling with this! Here is the data: Concentration of NaOH: .104M Mass of Aspirin #1: .367g Mass of Aspirin #2: .365g Volume of NaOH mixed with Tablet 1: 50ml Volume of NaOH mixed with Tablet 2: 50 ml Trial 1 Mass of Na2CO3: .065g Initial volume of HCl: 18.80mL Final Volume...

1) Given: 0.100 M NaOH, 5 mL concentrated acetic acid. 30 mL of distilled water was added to dilute the concentrated acetic acid. Calculated: Equivalence point (Vol = 32.5 mL, pH = 9.3) 1/2 equivalence = 32.5 mL/2 = 16.25, pH = 4.4 1. Calculate the concentration (M) of the diluted acetic...

Homework Statement :[/B] The percentage of copper in a Copper (II) salt can be determined by using a thiosulphate titration. 0.305g of a copper (II) salt was dissolved in water and added to an excess of KI solution liberating Iodine. The liberated Iodine required 24.5 ##dm^3## of a 0.1 mole...

Homework Statement :[/B] A mixed solution of KOH and sodium carbonate required 15ml of (N/20) HCl solution when titrated with phenolphthalein indicator. But the same amount of solution, when titrated with methyl orange as an indicator, required 25ml of the same HCl. The amount of KOH in the...

Homework Statement :[/B] 1.08g of ##NH_4 Cl## is boiled with 62ml ##\frac {N}{2}## ##NaOH## to expel ##NH_3## completely. 44ml of ##\frac {N}{4}## ##HCl## is required to neutralise the excess alkali. Calculate the percentage of ##NH_3 ## in ##NH_4 Cl##. Answer given: 31.5% Homework Equations...

What is the difference between valence factor and n-factor for oxidants and reductants? Take ##H_2O_2## as an example. What is the difference between the n-factor and valence factor for this compound? Also, how do I find the n-factor for any oxidant or reductant?

1. The problem statement, "all variables and given/known data A solution of nitric acid, HNO3, of concentration 100 g dm-3, can be used to artificially age wood. A sample of nitric acid was tested by pipetting 10.00 cm3 of the acid into a 250 cm3 volumetric flask and filled up with deionised...

I want to prepare murexide indicator for Ca measurement using EDTA titrimetric method. I am following the procedure set by the American Public Health Association (APHA), however, I only have murexide diluted with K2SO4 (1:250). I want to know if I can use this as a substitute, and if yes, how...

Homework Statement a) Determine the concentration of NaCH3COO. The volume of HCl used to reach the equivalence point is 25.05 mL, the concentration of HCl is 0.10 M, and the volume of NaCH3COO solution used is 10.0 mL. b) Using the initial concentrations of NaCH3COO and HCl, and a reliable...

We were doing O2 estimation by Winkler's method The procedure and reactions involved in this experiment are: Carefully fill a 300-mL glass stoppered bottle brim-full with sample water. Immediately add 2mL of manganese sulfate to the collection bottle. Add 2 mL of alkali-iodide reagent (NaOH +...

I was reading through the standard complexiometric method of determining hardness in water, and the procedure mentioned the use of the magnesium salt of EDTA. I looked up online to purchase this reagent but all I could find was disodium magnesium salt of EDTA. Are they one and the same? Thanks!

So for my IA, I dissolved a 1000mg vitamin c tablet in 355mL of water, took 20mL of it and diluted it to 100mL making it about 0.0032mol/L. I then added 5mL of 0.5mol/L potassium iodide, 5mL of 1.0mol/L hydrochloric acid and some 6 drops of 1 gram of starch dissolved in 100mL of water. I then...

We were measuring the amount of O2 dissolved in water by Winkler's method. Here's a link to the procedure and reactions: http://file:///C:/Users/SANJUKTA/Desktop/Downloads/Capture.PNG http://dropcanvas.com/6su7m/1 (The same is attached to this post) We had to use this formula: c(O2)...

Hey guys! So I have this chemistry problem which I'm finding very difficult. QUESTION: You have an unknown triprotic acid, H3X, and have titrated it with 22.53mL of NaOH. The pH of the unknown solution is 2.04 and the concentration is 48.028g/2L. While the concentration of the NaOH is...

Homework Statement I conducted a titration experiment in which 0.1g of KHP was dissolved in 50mL of distilled water and placed in an Erlenmeyer flask. I filtered a Ca(OH)2 solution (that was left out open on the lab benches for us to use) and put that into the burette and titrated. Ultimately...

In my analytical chemistry lab course my lab partner and I are trying to determine the percent calcium by mass of an antacid tablet by EDTA (mixed with 0.001M MgCl2) titration using an EBT inidcator. We have ran into a problem which is we've got poor results which we refuse to accept. Long story...

Hey guys! I have an exam tomorrow on back titration. Can i have some useful advice?

Homework Statement When a weak acid HA is titrated 75% of its endpoint, it has a pH of 5.25. Calculate its Ka. Homework Equations Ka = [H+ ][A- ]/[HA] [H+] = 10^-pH The Attempt at a Solution I found [H+ ] from the pH to be 10^-5.25 M. From the dissociation equation of HA, we know there is a...

Homework Statement Homework EquationsThe Attempt at a Solution If 50% of the acid has been neutralised, then there is 0.05 M of acetic acid left.Using Ka $$ 1.8*10^-5 = \frac {x^2}{0.05-x} $$ I get x = 0.00094 -log(0.00094) =3.02687 =pH This is not one of the answers provided. I think I...

Homework Statement Homework Equations Henderson-Hasselbalch Equation The Attempt at a Solution Sorry for the huge picture, but the number says 0.007558 mol. Is my ICE table correct? Equation: 7.42 = 6.85 + log((0.007558-x)/x) (0.007558-x)/x = 3.715 x = 0.00160 mol H+/(0.07483 L + 0.01339 L)...

Hi I am stuck on the following question. Outline a plan of an experiment to determine the percentage of iron present as iron(III) in a solution containing Fe3+(aq) and Fe2+(aq) ions. You are provided with zinc, a standard solution of potassium dichromate(VI) and dilute sulphuric acid. Zinc can...

In acid base titration, we try to neutralize the analyte by adding sufficient titrant and observing the color change in the indicator. But if the analyte is neutralized, then it must always be at ph 7. Why is it that we use indicator of different ranges to check equivalence point?