Calculate the concentration of Pd

Q: Ag* 0.0000133038 Cr 0.0000133038

A: Concentration of Ag+ = 0.0000133M  Concentration of Cl- = 0.0000133M

Q: The quantitative determination of N,H, with KIO, proceeds in a mixture of H,O/CCI, as follows N,H, +…

A: Endpoint: refers to the point at which the indicator changes colour in  titration. The endpoint is…

Q: 12-6. A 100.0 mL solution of 0.050 0 M M"* buffered to pH 9.00 was titrated with 0.050 0 M EDTA. (a)…

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Q: +3 2C0 (aq) + Cl ag) + 20H +2 Cl0 (ag) + H20 + 2Co (aq) [C1"] When [C10) - 2.00 M, [Co*) - 0.50 M…

A: The balanced reaction taking place is given as, => ClO- (aq) + H2O (l) + 2 Co2+ (aq) ------->…

Q: ▼ ▼ Part A 9.00x10-3 mol of HBr are dissolved in water to make 18.0 L of solution. What is the…

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Q: Calculate the standard potential, E", for this reaction from its equilibrium constant at 298 K. X(s)…

A: We have to calculate the Standard potential value.

Q: 0-18. a. Calculate the quotient [H;P04]/[H,PO,] in 0.050 0 M KH,PO4. b. Find the same quotient for…

A: 1. First of all we must know the basic formulaes.  PH= - log [H+]

Q: Part A. Effect of current (in Ampere) to the Amount Deposited on the Cathode at constant time and EM…

A: According to Faraday law :  W = ZIt  Where Z = E/F  => W = EIt/F  W = amount deposited  I =…

Q: 65 What is the minimum concentration of NH3 (mmol/L) needed to prevent Ağci(s) from precipitating…

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

Q: The following reaction occurs in aqueous acid solution: NO, + I- –→ I0, + NO2 In the balanced…

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Q: 16) 30.0 mL of 0.1 M Na-CO, solution was titrated against HCI (10 mL) to reach the bromocresol end…

A: 16) Given, For Na2CO3 solution: Concentration of Na2CO3 solution = 0.1 M = 0.1 mol/L Volume of…

Q: Calculate AG and the exponent value (the x of 10) for K, for the following reactions at 25°C: (a)…

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Q: Write the basic equilibrium equation for HS. Be sure to include the proper phases for all species…

A: Bronsted and Lowry concept of Acids & bases is used to write basic equilibrium equation as…

Q: 6. On what electrode and What mass (in gram) of chlorine gas could be released from a solution of…

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Q: 51 PM Wed Apr 19 ... ☎96% + 1. Write the chemical reaction for the titration of the filtered KHT…

A: The question is based on the concept of organic reactions. We  need to write the balanced chemical…

Q: H Redew i Conatant MISSED THIST Watch KCVa2 Read Secnon e3 You can cick on the Review ink t accese…

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Q: Calculate the molar solubility and Ksp of borax at each of the measured temperatures.  Equations…

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Q: (10-3 Triprotic systems) Find the pH of (A) 0.10 M H3His2+; (B) 0.10 M H2His+ ; (C) 0.10 M HHis;

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Q: IA Cancel RESET Done A weak monoprotic acid HX is 1.5 % ionized in a 0.25 M solution of the acid.…

A: Final answer is given in explanation please see from there.Explanation:Approach to solving the…

Q: Write the reaction that takes place when H30*(ag) is added to ution containing H,PO4(aq) and H,PO4…

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Q: B) Use this molarity and the initial pH of the ethanoic acid to calculate the equilibrium molarities…

A: The pH of a solution helps us to determine the acidity or alkalinity of a solution. The pH is…

Q: Protection Standard addition. The 5-31. water below which no adverse health effects are likely to…

A: Depending on the nation and the body that establishes these criteria, there may be differences in…

Q: 17) 25.0 mL of NaCl unknown concentration was titrated against 23.0 mL of 0.009 M AgNO3. Calculate…

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Q: Chloride ions are added to the Ag|Ag half-cell of the cell Ag|Agl|CuCu to precipitate AGCI (s). The…

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Q: 2+ Sn²+ (aq) + Cu(s) → Sn(s) + Cu²+ (aq) Hint: Carry at least 5 significant figures during…

A: For a non-spontaneous reaction, ∆G°>0 and K<1

Q: A solution is prepared at 25 °C that is initially 0.66M in trimethylamine ((CH3)₂N), (K(CH₂), NH). C…

A: The concentration of  = 0.66 MThe concentration of  = 0.17 MThe Kb for  = pH of the solution =?…

Q: Calculate the relative neutralizing value for a ground limestone with the following characteristics.…

A: Answer- Effective Neutralizing value (ENV)- Relative Neutralizing value-

Q: Table 1. Crystal violet Concentration Test tube   10.0 x 10-6MCV(mL)  DistilledH2O (mL)…

A: The given table is:

Q: What is the pH of 0.43 M NH3 solution? (Kb = 1.8 x 105) NH, (aq)+ H,0 (1) NH (aq) + OH (aq)

A: Answer: pOH of solution is equal to the negative of logarithm of hydroxide ion concentration of it…

Q: Calculate the pH of 0.042 M HNO2 solution (Ka = 4.5 x 10 "). HNO, (aq) H' (aq) +NO; (aq)

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Q: 6. What is the N of 0.45 M Mg(OH)2

A: 6.) N ( normality ) and molarity are related to each other for give Compound type.

Q: Part A Calculate [H3O*] in the following aqueous solution at 25 °C: [OH¯]=1.0x10-9 M . Express your…

A: Ionic product for water Kw at 25oC is considered as 1.0x10-14 The expression for Kw is as shown…

Q: Find the equivalence point volume for both of the "good" trials. This will be most obvious using…

A: The sigmoidal curve observes for a combination of weak acids and strong bases or strong acids and…

Q: What is the smallest whole-number coefficient for H₂O when the equation MnO4 + 1 + H₂O → MnO2 + 103¯…

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Q: An ion-selective electrode (ISE) produces voltage output (mV) proportional to solution pH. You have…

A: The objective of this question is to show the pH 7 buffer solution serves as a reference for both…

Q: What would the potential of a standard hydrogen electrode (S.H.E.) be under the given conditions? H…

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Q: 17. The actual design of the indicator electrode referred to the pH electrodes cell, in the…

A: Electrochemistry is branch of chemistry in which we deal with oxidation and reduction reaction…

Q: An aqueous solution at 25 °C has a OH concentration of 3. x 10 M. Calculate the H,0' concentration.…

A: To find out H3O+ concentration, use the formula which contains Kw, H3O+ and OH- in it and solve for…

Q: Percent Ca in unknown

A: In order to determine % Ca in unknown, we must first determine the amount of Ca in each ppt.

Q: If [H3O*] = 3.8 x 10-3 M, what is the pOH of the solution? %3D O 2.42 O 2.13 O 2.77 11.58

A: The given data contains, H3O+=3.8×10-3M.

Q: Standard Solutions and Determination of ɛ Use the slope and the path length to find the molar…

A: Using beer Lambert's law             ε  or molar extinction coefficient and it  is a measure of…

Q: 8-13. Using activities, calculate the pH of a solution containing 0.010 M NaOH plus 0.012 0 M LINO3.…

A: The explanation is given below-

Q: 1. Prediction of pH and hydrolysis of salts: Aqueous Solutions NH4CI NaCI Na2CO3 CUNO3 NaC2H3O2…

A: Given : Incomplete table of prediction of pH value.  To find : PH of compounds is nature of the…

Q: Create a calibration curve. Electrode potential (mV) vs. log [Ca2+]. (complete with, the equations…

A: A question based on tools in analytical chemistry that is to be accomplished.

Q: Pt / UO22+ (7,90x10-3 M), U 4+ (9,18x10-2 M), H* (1,47x10-3 M) // Fe* (1,28 x 10-M), Fe* (2,84 x…

A: In the given cell apply Nerst equation and determine Ecell  and if Ecell is positive then cell is…

Q: Part C. Effect of Equivalent mass (EM) to the amount deposited on the cathode at constant current…

A: Electrolysis It is the process of decomposition of electrolyte by passing electric current through…

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red. 

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.