Lab 5 - seperation (fall 2023)

Calculate the total volume of HCl titrant delivered to the equivalence point for each trial

A student has been asked to prepare a reaction mixture, which is suitable to test the activity of an enzyme in dependence of the pH of the solution. The mixture contains a buffer compound, which will facilitate a stable pH. Now they have to determine the ratio of conjugate base/weak acid required such that they will obtain the desired pH. They have been provided with the buffer parameters provided in the image below. Determine the ratio with two decimal places precision. B_A ratio_007 Note: You may need to round the numbers to get the required answer. Previous Page Next Page Final pH of solution: 5.8 Final volume of solution: 100 ml Buffer compound concentration: 150 mM Buffer compound pk₂: 6.3 Page 4 of 12

Write the Ksp expression for the sparingly soluble compound silver cyanide, AgCN. If either the numerator or denominator is 1, please enter 1. Ksp = Submit Answer Retry Entire Group 8 more group attempts remaining

(4c-201) Copy the following equation, and label the Bronsted-Lowry acid, its conjugate base, the Bronsted-Lowry base, and its conjugate acid. HNO3 + H2O → H30* + NO3¬ For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). BIUS Paragraph Arial 14px A v ... In X2 田由田図 EX: ABC Ť {;} > >

Ksp for PBF2(s) is 3.3 x 10-8. Write the chemical reaction that occurs when PBF2(s) partially dissolves in water. Include physical states in your answer. eTextbook and Media Save for Later Attempts: 0 of 3 used Submit Answer

Qualitative Analysis Step 2. The solubility of lead is sufficiently high that at low lead concentrations, all of the in addition, the solubility of lead increases about threefold in hot water compared to room tem perature water; thus, a significant amount of lead can be solubilized from the mixture of AgCl, H92CI2, and P6CI2 by treating the mixture with hot water. Therefore, centrifuging the resulting solution leaves only a solution of lead (if lead is present). Step 3. The presence of lead can be confirmed or eliminated by the addition of chromate to form the bright yellow solid PbCrO. (Equation 8). You may recognize this color because lead chromate is often the pigment in the yellow paint used to paint yellow lines on highways. Equation (8) Pb2*(aq) + Cro?-(aq) PbCrO4(s) Ksp = 1.8 × 10-14 Step 4. The addition of aqueous ammonia results in the formation of the complex ion [Ag(NH3)21*, solubilizing the silver, but also in the disproportionation of the Hg* (i.e., Hg2") into Hg° metal…

Please answer letter c

M1= 25mL p

i need help calculating the molar concentration for part C

UPLE Using the following data, determine the pH and ionization constant of acetic acid. Procedure and Parameters Initial volume of 0.100 M acetic acid added Volume of distilled water used Conductivity of distilled water Conductivity of the prepared acetic acid Molar conductivity of acetic acid at infinite dilution Results 5.00 mL 50.00 mL 8 μµS.cm-¹ 165 µS.cm-¹ 3.955 x 105 μS.cm-¹-M-¹

please help me answer this one, thanks.

Part IV: Equilibrium Involving Chromate and Dichromate Ions Steps 2 & 3 Step Steps 5 & 6 4 Steps 7 & 8 Step 9 2CrO₂² (aq) + 2 H (aq) Cr₂O, (aq) + H₂O (1) Initial Colour + 1 M NaOH + 1 M HC1 Ba² (aq) + CrO² (aq) BaCrO. (s) 0.1 MK₂CrO₂ Yellow Yellow Yellow Initial Colour + 1 M HC1 + 1 M NaOH 0.1 MK₂CrO₂ + 0.1 M Ba(NO3)2 Other Observations: 0.1 MK₂CrO₂ Yellow Orange Yellow Initial Colour Yellow 0.1 MK₂Cr₂O, Orange Initial Colour + 1 M NaOH Yellow + 1 M HC1 Orange 0.1 MK₂Cr₂O, Orange Yellow Orange 0.1 MK₂Cr₂O₂ + 0.1 M Ba(NO3)2 Orange Orange Orange Immediately cloudy with white precipitate and yellow solution + 0.1 M Ba(NO₂)₂ Orange + 1 M HC1 Orange with precipitation + 1 M NaOH Yellow with precipitation 0.1 MK₂CrO₂ 0.1 MK₂Cr₂O, Immediately a lot of precipitate Very little precipitate formed in formed in yellow solution orange solution

The calcium ion binds to a certain protein to form a 1:1 complex. The following data were obtained in an experiment. Total Ca2+/µM 60.9 122 186 250. 536 Ca2+ bound to Protein/µM 31.4 51.4 63.6 71.0 83.6 Determine graphically the dissociation constant of the Ca²+-protein complex. The protein concentration was kept at 97 µM for each run. (1 µM = 1x10-6 M.) Kd =

* 10.04 pH and Acidity: Introducti x 101 Chem101 b Search results for 'Complete the x A app.101edu.co Question 15 of 35 Submit Complete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. CH;NH2(aq) + HCIO;(aq) - 4- O3- D2- O2+ 3+ D4+ 1 2 4 6. 7 1 3 4 7 8 (s) (1) (g) (aq) OH- C H N H20 Reset • x H2O Delete 1L

Please ! Do both neat and clean correctly on a plain white paper please... Don't paste irrevelant answer to waste my question otherwise be ready for getting reported to the team.

11. A solution of Na₂SO, is added to a solution that is 0.010 M in Ba2+ and 0.010 M in Sr2+. The Ksp of BaSO4 = 1.1 × 10-10 and the Ksp of SrSO₁ = 2.8 x 107 a. 2- Bq²++ S04² = Basoy +504 Sp2t+ Sou² Sr504 What molar concentration of sulfate ion is necessary to begin precipitation? 72 ksp=[B₁²+]² [sout]² [So²] = k sp Ba 10 1.1x10 0.01 1.1x10-8 M Sr [So₁7] = \3P 2.8×10-7 0.01 = 2.8×105 M b. Which of the 2 cations will be precipitated first? C. What is the sulfate ion concentration when the second cation begins to precipitate?

I need help calculating the remaining values please!!!!

Ooldtion Table 1. Measurements for standardization of NaOH Trial 1 Trial 2 Trial 3 1] Tared mass of KHC3H4O4 (9) 0.374 0.325 0.357 12] Burette reading of NaOH, initial (mL) 4.59 3.61 4.03 [3] Burette reading of NaOH, final (mL) 22.03 18.77 21.17 Part B. Molar Concentration of an Acid Solution Enter the number corresponding to the type of acid you have 1. HA 3 2. H2A 3. H3A Enter the unknown number. 21 Table 2. Measurements for titration of unknown acid Trial 1 Trial 2 Trial 3 [1] Volume of acid (mL) 25.0 25.0 25.0 [2] Burette reading of NaOH, initial (mL) 2.13 2.48 3.68 [3] Burette reading of NaOH, final (mL) 24.10 24.52 25.56 Part C. Percentage by Mass of an Unknown Solid Enter the number corresponding to the type of acid you have 1. HA 3 2. H2A 3. H3A Enter the unknown number. 30 Molar mass of the unknown acid 192.14 Table 3. Measurements for titriation of solid Trial 1 Trial 2 Trial 3 [1] Mass of sample (g) 26.334 29.157 27.111 [2] Burette reading of NaOH, initial (mL) 3.21 1.48…

Pls help ASAP. Pls show all work and calculations.

< = 2 = 3 Ksp = 0 = 4 = 5 = 6 Complete the following solubility constant expression for CaCO3. = 7 X 00 S 010 8

Only number 11 that u have to do

Explain how it is that SPE cartridges & disks allow analysts to more efficiently pre- concentrate analytes from samples where they exist at low concentrations.

I am confused on how to do one and two? Help please.

Pls do fast within 5 minutes and i will give like for sure AP Chemisty KSP

Your pH meter was improperly calibrated and reports a pH value consistently lower by 0.002 compared to the correct value. This discrepancy introduces error to your data. systematic random

4. To perform a certain activity assay it is necessary to have 0.25 mL of an enzyme at a concentration of 0.2 mgml¹ in the presence of 0.4 mM substrate and 200 mM NaCl in a suitable buffer. The stock solutions of enzyme, substrate and NaCl are 4 mgmL-¹, 40 mM and 1 M all in the same type of buffer. What volumes of the stock solutions and buffer are required for each assay?

I need the answer for this question as Sage Math Code. It's a linear algebra

ns 画 ది 3/4 Georgian Q49 (Ex. 13.6) In chemistry, the pH value .. measure.. acidity. The pH value is defined by pH = – log(H*) where H*is the hydrogen-ion concentration (in mol/L). If the pH of rainwater is 4.764, find the hydrogen- ion concentration. (If pH 7, solution is basic.) SOLVING EXPONENTIAL EQUATIONS To solve... 1. Isolate... 2. Then do ... (?) = log(number) or (?) = In(number) or (?) = loga(number) 10?) = (number) e(?) = (number) a(?) = (number) 012/5

Q12 Needed ASAP

What conclusion can be derived from the following sentences regarding analytical methods: I. Classical methods (gravimetry and volumetric methods) are no longer useful in analytical chemistry. II. Volumetric methods do not require calibration if a primary standard is used as titrant. III. Instrumental methods are useful with analyte solutions that are less than 1.00 mM. IV. Classical methods yield high precision and accuracy at concentrations greater than 1.00 mM. What conclusion can be derived from the following sentences regarding analytical methods:   Two statements are incorrect. All statements are correct. One statement is incorrect. Only one statement is correct. All statements are incorrect.