Answer the following questions regarding a 50.0 mL solution of 0.100 M solution of a weak acid, HY, Ka = 1.80 x 10-8 . The solution is titrated with o.100 M NaOH.   a. Calculate the volume of base needed to reach the equivalence point.       b. Calculate the pKa for the weak acid.       c. Determine the pH of the original acid solution.     d. Sketch a titration curve for this experiment, (You can insert a graph or write on a graph paper paper)

Q: 2. Describe how you would go about in the lab making 100 ml of a buffer solution of 0.10 M acetic…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: 3.) What is the pH at the equivalence point for the titration of 50.0 mL 0.20 M nitrous acid by 0.20…

A:

Q: 1. You have a 50.0 mL buffer that is 0.500 M in both A- and HA. The pKa = 5.00. a) What is the…

A: Handerson-hasselbalch equation is used to calculate the pH of the buffer system. here is the acid…

Q: .) An experiment similar to the one performed was done in order to determine the Ksp of Ba(OH)2. In…

A: Given Base Ba(OH)2 Acid (HCl)when we mix them acid base neutralisation reaction occur and we get…

Q: Bicarbonate Buffer a. Prepare 100 mL of 0.200 bicarbonate buffer, pH 10, by calculating the mass of…

A: a-Method I-Prepare a 0.2M arrangement of anhydrous sodium carbonate of 50 ml w = (mw*V*0.2)/1000 w =…

Q: a. Find the pH of a solution that is 0.600 M in formic acid and 0.400 M in sodium formate. Ka…

A:

Q: A solution containing 100.00 mL of 0.1800 M acetic acid (Ka = 1.78 x 10-5) is being titrated with…

A: GIVEN: Volume of acetic acid= 100.0 mL Concentration of acetic acid =0.1800 M Concentration of NaOH=…

Q: Consider the titration of 75.00mL of 0.235 M nitrous acid (HNO2) with a 0.600 M KOH solution. a.…

A:

Q: 3. A buffer was prepared by mixing 19.53 g NaF and 10.41 g HF in a 1.0 L reaction vessel. Ka = 7.1 x…

A:

Q: This question concerns part 1 of this lab. You need to make a buffer solution by mixing both a weak…

A: Let's create a buffer solution using acetic acid (CH₃COOH) and sodium acetate (CH₃COONa). The goal…

Q: Calculate the pH of a buffer that is 0.020 M in NH3 and 0.030 M in NH4Cl. What is the pH after…

A: The pH of a solution can be expressed as the negative logarithm of hydronium ion concentration.i.e.,…

Q: A 0.544 g sample of a diprotic acid with a molar mass of 255.8 g/mol is dissolved in water to a…

A: Mass of diprotic acid = 0.544 gMolar mass of acid = 255.8 g/molTotal volume of acid solution = 28.0…

Q: The names and chemical formulae of some chemical compounds are written in the first two columns of…

A:

Q: a. Find the pH of a solution that is 0.750 M in formic acid and 0.400 M in sodium formate. Ka…

A: a)The given question can be solved by using Handerson Hasselbach equation- pH = pka + log…

Q: Xanthoproteic Test To 2 mL of sample add 1 mL concentrated HNO3. Observe whether a heavy white…

A: A question based on qualitative analysis, which is to be accomplished.

Q: Given a buffer of Lactic acid (0.15 M) and sodium lactate (0.25 M) and that Ka is 1.4 x 10-4. a .…

A: Given : Concentration of Lactic acid i.e HA (monoprotic acid) = 0.15 M Concentration of sodium…

Q: For the titration of 30.0 mL of 0.250 M NH3 with 0.500 M HCl at 25 °C, determine the relative pH at…

A:

Q: 4. A buffer was prepared using 10.0 mL of 1.90M HAc and 1.20 M NaAc (where Ac- is C2H3O2- ). The Ka…

A: Buffer solution are those who resist the change in pH of solution on small addition of strong acid…

Q: 2. 100.0 mL of a 0.0875 M weak base solution is titrated with 0.250 M HCI. The pH after the addition…

A: Given,  Concentration of weak base (say B) = 0.0875 M  Volume of B in mL = 100.0 mL  Concentration…

Q: A buffer is made by dissolving 21.5g of benzoic acid, HC7H5O2 (Ka = 6.4 x 10-4) and 37.7g of sodium…

A: Given: The Ka of benzoic acid = 6.4 × 10-4 We have to calculate the pH of a buffer made by…

Q: The curve shown was produced during the titration of a 15-mL sample of a weak acid, HA, with 0.10 m…

A: At the equivalence point, the number of moles of NaOH is equal to the number of moles of HA acid.…

Q: Using Titration to Determine the Identity of an Unknown Acid 5. An unknown acid is titrated with…

A: The above titration curve look like weak achid vs strong base (NaOH). From Henderson-Hesselblech…

Q: In which solution would you expect zinc hydroxide to be the most soluble given that Ksp of Zn(OH)2…

A: 1 M  strong base

Q: 8. Calculate the volume of 1.0M acetic acid and 1.0M sodium acetate solution needed to make 250 mL…

A: Given that, Molarity (concentration) of acetic acid = 1.0 M Molarity of sodium acetate = 1.0 M…

Q: . What is the pH of the solution obtained when 25.0 mL of 0.065M benzylamine, C7H7NH2, is titrated…

A: Given Concentration of benzyl amine = 0.065 M Volume of benzyl amine = 25.0 mL Concentration of HCl…

Q: Titration of another 30.0 mL sample of aqueous HX with 0.111M NaOH yields the titration curve below.…

A: A) 1 mole of NaOH used to neutralize 1mol of acid.  NaOH + HX ------> NaX + H2O  30 ml of NaOH OF…

Q: a. Calculate the pH of a saturated solution of Ba(OH)2. Ksp = 5.0 x 10-3 pH = b. Calculate the pH of…

A: (a) The given information is as follows:             Ksp of a saturated solution of BaOH2 = 5.0×10-3…

Q: 9. Consider the titration of a sample of a weak acid with a strong base (titrant). What is the…

A: 9. A weak acid is titrated with a strong base.  Here, we have to select the correct option for the…

Q: Use the titration curve for the weak acid to calculate the pH of a 0.150 M solution of that weak…

A: The pKa of the acid will be equal to the pH at half equivalence point which can be determined by…

Q: What is the Ksp expression for the dissolution of Ca(OH)2? Ksp = [Ca2+] + [OH−] Ksp = [Ca2+] +…

A: We have to predict Ksp expression for Ca(OH)2 , also the relation in Ca+2 and OH- .

Q: Select the mixture which is capable of tolerating addition of a strong acid without altering the pH?…

A: Choose a mixture which act as a buffer to resist to change  a PH of a solution ? Adition of strong…

Applications of Molecular Spectroscopy

When light sources pass through the diffraction grating then light splits into different wavelengths. The light source produces two types of patterns that are shown as destructive and non-destructive. The light source is in the form of quanta that is quantitation.