Answered: Q2) Q2) How much mole of NH3 to be…

Q2) Q2) How much mole of NH3 to be added to 500 mL of the solution with pH=8.9 to dissolve 5x10 * of AGSCN? PKSP(AGSCN)=12 , PKa(NH.) =9.2 , PKdAg(NH3)**/Ag+=7.2

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 4RQ: A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If...

See similar textbooks

Related questions

Q: Look at Figure 2.17. If you did this titration using TRIS instead of phosphate, how would the…

Q: 6. Calculate volume in ml of 0.200 M NAOH solution required to neutralize 1.858 g of primary…

Q: At temperature 25°C, 0.02 M hydrazine, N2H4 solution is 0.69% ionised. Calculate the i.…

A: Since you have asked multiple question, we will solve the first question for you.If you want any…

Q: The pk, for the acid dissociation reaction of bicarbonate is 10.33. HCO3 (aq) + H2O(1) 2 CO32-(aq) +…

Q: 3. Calculate the (a) pH (b) pOH (c) percent ionizaton of 0.100 M ammonia. NH3 kb = 1.8x10^-5

A: Since, you have asked multiple question, we will solve the first question for you. If you want any…

Q: Using the systematic method, determine the molar solubility of AgBr(s) in a) water b) 0.15 M NaBr c)…

A: Here we have to determine the solubility of AgBr at different conditions i.e a) in pure water b)…

Q: how to prepare this buffer TES (Sigma-Aldrich) infiltration buffer (10 mM TES, 10 mM MgCl2, pH 7.5)…

A: TES, having the molecular formula C6H15NO6S, is widely used to prepare buffer solution. A TES buffer…

Q: Calculate the volume, in milliliters, 0.170 M NaOH that must be added to 303 mL 0.0471 M…

Q: Why do you have to titrate until or above pH = 12.5 ± 0.2 to properly identify the unknown acid…

A: by titration we can get the quantitatively amount of the acid solution .

Q: Calculate Q for the following: 125.0 mL of 0.0800O MPb(NO3)2 is mixed with 75.0 mL of 0.0200 MNACI…

Q: 2. In the pH metric titration of strong and weak acid mixture against strong alkali, generally first…

A: We are given a mixture of strong acid(H+) and weak acid(HA). We titrate the above mixture with a…

Q: CrO42- can be used as an indicator when Br- is titrated with Ag+. What concentration of CrO42-…

Q: What volume (V) of 0.100M (moles) KMnO4 would be required to Titrate 0.23g of…

A: The volume (V) of 0.100M (moles) KMnO4 is to be calculated.

Q: Calculate the volume, in milliliters, of 0.170 M NaOH that must be added to 305 mL 0.0409 M…

Q: A 15.00 ml aliquot of a 0.75 M solution of a weak acid (K, = 1.50E-05 at 25°C) is titrated with…

Q: Use the Solver function in Excel to determine [Sr²+], [F¯], [HF], [OH-], and [H*] for a saturated…

A: Introduction: Solubility product: Solubility product constant measure the extent to which a solute…

Q: What is the function of the vacuum aspirator? Predict the color shift of the indicator as a…

A: Aspirator is a tool which uses suction to remove or collect something specially in medicine for…

Q: Which of the following statements is advantageous? A). The main differences between potentiometric…

A: The major difference between potentiometric and conductometric titration is that potentiometric…

Q: The pH of a 0.2L HNO2-NO2 buffer solution was determined to be 6.23. The solution was mixed with…

A: Buffer solution A buffer solution is an aqueous mixture of a weak acid and either its conjugate base…

Q: if wc dissolve an acid dissolve an a cid weak HzA in wate, t he solution volume will be loomb, and…

A: 1- First determine the concentration of H+ ion : We know that, pH = -log([H+]) -pH = log([H+])…

Q: You are asked to prepare 500. mL 0.300 M acetate buffer at pH 5.00 using only pure acetic acid (MW =…

A: This problem can be solved using the Henderson Hasselbalch equation. It states the relation between…

Q: Consider the reaction of 75.0 mL of 0.350 M C₅H₅N (Kb = 1.7 x 10⁻⁹) with 100.0 mL of 0.393 M HCl.…

Q: It has been found the azide (N3-) forms an "insoluble" compound when in the presence of lead, which…

A: Pb(N3)2 = Pb2+ + 2N3- if solubility is s then: Pb(N3)2 = Pb2+ + 2N3-…

Q: Titration of 0.1756 g of primary standard Na2C2O4 (anhydrous) required 32.04 mL of a potassium…

Q: Consider the reaction of 75.0 mL of 0.350 M C₅H₅N (Kb = 1.7 x 10⁻⁹) with 100.0 mL of 0.425 M HCl.…

A: Given: Volume of C₅H₅N = 75.0 mL Concentration of C₅H₅N = 0.350 M Volume of HCl = 100.0 mL…

Q: 3-2 How many moles of NH,CI must be added to 2.0 L of 0.1M NH, to form a buffer whose PH of 9.00 ?…

A: The given data contains, Volume of ammonia =2.0 LConcentartion of ammonia=0.10M pH =9pKb =4.75

Q: 7.2 Four pK, values (1.0, 2.0, 7.0, 9.0) are tabulated for the acid H,P,0,. Write equations to show…

A: pKa values are correspond to negative logarithm of dissociation constant, i.e., higher the value of…

Q: A 15.00 ml aliquot of a 0.75 M solution of a weak acid (K, = 1.00E-05 at 25°C) is titrated with…

Q: A buffer was made by mixing 0.1404 moles of HN3 with 0.1025 moles of KN3 and diluting to exactly 1…

A: Given: Ka(HN3) = 1.9 x 10-5 pKa(HN3) = 4.72

Q: 3. The maximum buffering capacity is nearest to the pka of the buffer. Explain why?

Q: Imidazole (C3H4N2, MW = 68.07816, Kb = 9.80 x 10–8) can be used to create buffers at physiological…

A: Buffer are solution which resist change in PH when acid Or base are added

Q: 00 50 10.0 15.0 20.0 25.0 30.0 Volume of NaOH (mL) Data colected during the titration of a 20.0 m…

A: From the graph Total volume of NaOH used for Titration = 20 ml = 0.020 L Volume of Acid =…

Q: The Ka values for nitrous acid (HNO2) and hypochlorous (HClO) acid are 4.5 x10-4and 3.0 x10-8,…

A: The pKa values of HNO2 and HClO is calculated below. The pKa of HClO is closer to the required pH…

Q: How much pH should be at least for Cr(OH)3 to collapse from a solution containing 0.076 M CR3+…

Q: Phenol red is a common acid-base indicator. It has a pKa equal to 8.000. Its undissociated form is…

A: Solution a)

Q: A microbiologist is preparing a medium on which to cultureE. colibacteria. She buffers the medium at…

A: To calculate the volume of the equimolar aqueous solution of K2HPO4 and KH2PO4 that must be combined…

Q: Suppose titration of 100.00 mL mixture of 0.0500 M in Br +0.08 M CI with 0.4000 M AgNO3. What is pAg…

A: Please find the below attachments.

Q: To prepare 1 liter of 0.10 M acetate buffer at PH 5.20.I need to mix _____g of CH3COONa molecular…

A: Any particular amount of acidic species or basic species which is added to any buffer solution…

Q: When a drop (taken to be 0.20 cm3) of 1.0 M HCI(aq) is added to 25 cm3 of pure water, the resulting…

A: Calculate the number of moles of HCl, ethanoic acid and sodium ethanoate. Number of moles =…

Q: In a lab, dissociation constant, K, of an acid-base indicator is measured. A 1.00 x 104 M solution…

A: Concentration (C) of the indicator = 1.00 x 10-4 M path length (l) of cuvette = 1.00 cm Molar…

Q: An analytical chemest is titrating 150.6 ml. of a 0.6600 M solution of dhethylamine (C,H,), NH) with…

Q: A 15.00 ml aliquot of a 0.75 M solution of a weak acid (K, = 1.50E-04 at 25°C) is titrated with…

Q: pH of solution made by mixing 200 mL of 0.2 M CH3COONA and 400 mL 0.1 M CH3COOH is [pKa(CH3COOH) =…

A: This problem can be solved by using the Henderson hasselbalch equation which may be expressed as:…

Q: 4. A 100.0-mL solution consisting of 0.14 M NaC2H30z and 0.16 M HC2H302 was titrated with 24 mL of…

A: 4. Millimoles of KOH = M x V = 0.25 x 24 = 6 mmol Millimoles of HC2H3O2 = M x V = 0.16 x 100 = 16…

Q: If 21.6 mL of 0.107 M acid with a pKa of 5.16 is titrated with 0.105 M NaOH solution, what is the pH…

A: According to Henderson - Hasselbalch equation: pH=pKa+log[conjugate base][weak acid] At, half…

Q: A student pharmacist prepared a buffer solution by mixing 68 ml of 0.17 M ammonia and 42 mL of 0.12…

Q: Calculate the volume, in milliliters, of 0.170 M NaOH that must be added to 247 mL 0.0581 M…

Q: pH indicator. A dye that is an acid and that appears as different colors in its protonated and…

Q: Lead sulfate is a mostly insoluble salt. The equation for the minimal dissolving of this salt is:…

A: We will answer this question using the common ion effect.

Question

Q2) Q2) How much mole of NH3 to be added to 500 ml of the solution with pH=8.9 to dissolve 5x10
* of AgSCN?
PKSP(AGSCN)=12, PKa(NH.') =9.2 , PKDA9(NH3)*/Ag+=7.2

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

3. A solution was prepared by adding 4.95 g sodium acetate (NaC;H;O2) to 250.0 mL of 0.150 M acetic acid (K = 1.75 x 10). Assume negligible volume change. a) What is the pH of the resulting solution? PH: pk2 + log CH3 02) moles saium 4.959 0.06 mol %3D 2cent %3D 82gmu H: -log (1.73x 10) + log 0.24 moles 2cete 250 x 0.15 IL :00375 1000me PH : 4 1.96 O.06 (N2 G Hs0): 0.24m 0.230 L O.0375 : CCHS COOH): 0 15 m Assume 125.0 mL of the solution prepared above was put into a beaker and 82 mg of NaOH was added to it. What is the pH of this new mixture? b)
1. Calculate [H+], [OH-], pH and pOH of:a. 0.1 M HNO3 b. 2.00 M (weak acid) HF (Ka=6.8 x 10^-4) 2. In the preparation of the standard curve for protein analysis, 50 mnBSA (bovine serum albumin) dissolved in H2O to a final volume of 5mL was used as stock solution. What is the weight of BSA in 0.1 mL ofstock solution? In 0.2 mL? 3. . The above mentioned aliquots (#9) which were diluted with enoughwater to a final volume of 1 mL were assayed colorimetrically andyielded the following absorbance readings:mL stock mL H2O Absorbance0.2 0.8 0.1000.4 0.6 0.2000.6 0.4 0.3000.8 0.2 0.4001.0 0.0 0.500 i. Tabulate mg BSA vs. absorbance readingii. Draw the curve where mg BSA is on x-axis and absorbance ony-axis (use graphing paper).iii. Calculate the slope of the curveiv. If a sample solution has an…
3. Complete neutralization of 10 ml of phosphoric acid solution by NaOH 0.I N in the presence of phenol phthalein until the appearance of purple color (pH, = 9) 11 ml. of NaOH is consumed. (a) What is the concentration of phosphoric acid? (b) Calculate the indicator error. pk2.1 pK. - 7.2 pK - 124
please answer on 1-a,b,c,d. Clear handwriting or type in, thank you! 1. The mixture of anions is an effective blood buffer with the following acid-base equilibrium: HO" (aq) + HPO* (aq) H:POs (aq) + H;O (1) a. For the equilibrium above, what is the effect of decreasing the pH? (give shift) b. As a result of the shift, which ion H:PO, or HPO, would appear to increase? c. For the equilibrium above, what is the effect of increasing the pH? (give shift) d. As a result of the shifl, which ion H:PO, or HPO would appear to increase?
A buffer solution after the addition of 20.0 mL of 1.00 M NaOH solution to 500.0 ml ot a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30 M sodium acetate (CH3COONA). [Ka= 1.8 x 10-1 What is the new concentration of the conjugate base, CH3COO after buffering? 0.3385 0.2434 0.1172 0.2269 0.4287
Direction: Solve for the pH or pOH of the following buffer solutions using the Henderson-Hasselbalch Equation. 1. Find pH for buffer 0.12 M HNO2, 0.16M NaNO2 with the given Ka (HNO2)= 4.5x104.
(5e) Which two of the following compounds would you make a buffer of pH = 12.5. H3PO4 (MM=98.00 g/mol), NaH2PO4 (MM=119.98 g/mol), NazHPO4 (MM=141.96 g/mol), and Na3PO4 (MM = 163.94 g/mol)? [For H3PO4: pK; = 2.148; pKz=7.199; pK3=12.15]
(а) A student mixed 200 mL of 0.15 M ammonium chloride, NH4CI with 200 mL of 0.23 M ammonia solution, NH3. i) Calculate the pH value of the mixture. 11) Calculate the concentrations of OH in the mixture. [K, for NH3 1.8 x 10 ] (b) Consider a titration between HNO; and NH3, i) write the reaction equation for this titration. ii) sketch the titration curve if the burette contains NH3 and colonical flask contains HNO:. in) classify the salt as neutral, acidic or basic ....
If the standard solutions had unknowingly been made up to be 0.0024 M AgNO3 and 0.0040 1 MK2CrO4, what would be the value of Ksp? The value of Ksp would be larger. The value of Ksp would be smaller. The value of Ksp would be the same. O More information is needed to answer this question.
Aniline, abbreviated fNH2, where f is C6H5, is an important organic base used in the manufacture of dyes. It has Kb = 4.3 * 10 - 10. In a certain manufacturing process it is necessary to keep the concentration of fNH3+ (aniline’s conjugate acid, the anilinium ion) below 1.0 * 10 - 9 M in a solution that is 0.10 M in aniline. Find the concentration of NaOH required for this process.
Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH,);N (K, = 5.2 x 10-4), with 0.1000 M HCl solution after the following additions of titrant. (a) 13.00 mL: pH = 10.305 (b) 20.10 mL: pH = (c) 29.00 mL: pH = %3!
Calculate the pH at the equivalence point in titrating 0.077 M solutions of each of the following with 0.068 M NaOH. (a) hydrochloric acid (HCl) pH = (b) arsenous acid (H3AsO3), Ka = 5.1e-10 pH = (c) hydrazoic acid (HN3), Ka = 1.9e-05 pH =