[Cu2+] at equilibrium

Q: Calculate the [Ag+] in a solution prepared by dissolving 1.00 g of AgNO3 and 10.0g KCN in enough…

A: Reaction: Ag+ +2CN- ⇋ [Ag(CN)]- 1 mole of AgNO3 reacts with 2 moles of KCN to form 1 mole of…

Q: A 0.170 mol quantity of CoCl, is added to a liter of 1.20 M NH, solution. What is the concentration…

A: Solution: 1) 0.170 mole of NiCl2 is added to a liter of 1.20 M NH3 solution. Therefore, the…

Q: A buffer solution that is 0.461 M in HClO and 0.461 M in NaClO has a pH of 7.46.

A:

Q: Use the Henderson–Hasselbalch equation to calculate the pH of a buffer solution that is 0.50 M in…

A: Henderson-Hasselbalch equation Henderson-Hasselbalch equation explains the relationship between pH…

Q: Write the net ionic equation for the [CoCl4]?- ion/[Co(H2O),J²+ ion equilibrium.

A:

Q: The molarity of an EDTA solution is 0.0114 M.  A 25.0 mL sample of water with unknown Ca+2…

A: Molarity is number of moles of solute present in 1 liter of solution. Mass of substance = molar mass…

Q: Calculate [Cr3+] in equilibrium with Cr(OH)4-(aq) when 0.010 mol of Cr(NO3)3 is dissolved in 1 L of…

A: Equilibrium constant (K) is the expression to relate the products and reactants of a chemical…

Q: A buffer solution is prepared in which the concentration of NH3 is 0.20 M and the concentration of…

A: Given : buffer solution of weak acid NH4+ and its conjugate base NH3  concentration of NH3 = 0.20 M…

Q: Calculate the solubility product for the following: a. 0.005 M CaSO4 b. 0.125 M Ag2CO3 c. 0.0450…

A: a. 0.005 M CaSO4 b. 0.125 M Ag2CO3 c. 0.0450 M Cr(OH)3

Q: Calculate the molar solubility of Ag2CO3 in a solution buffered to a pH of 7.50

A: In The above question molar solubility of Ag2CO3 have to be determine in pH7.50.

Q: Find [Cu+] in equilibrium with CuBr(s) and 0.10 M Br2.

A: Concentration of Br2 = 0.10M Ksp of CuBr = 5 × 10-9

Q: What is the solubility of Cr(OH)₃ at a pH of 10.90? (Ksp Cr(OH)₃ is 6.70 × 10⁻³¹)

A:

Q: If 2.13 g of CusO4 are dissolved in 9.0 × 102 mL of 0.30 M NH3, what are the concentrations of Cu2+,…

A: Moles of CuSO4 = Mass/Molar mass = 2.13g/(159.6g/mol) = 0.0133moles Volume = 9.0 ×102 mL = 0.9 L…

Q: 13. When dilute HCl is added to a solution, a white precipitate forms. Which ion was likely in the…

A:

Q: You have been given an unknown that contains a Group I ion (Ag+ or Hg22+), a Group II ion (Fe2+ or…

A: Hey, since there are multiple questions posted, we will answer the first question. If you want any…

Q: Calculate the concentration of Sr^ 2+ when SrCr * O_{4} starts to precipitate from a solution that…

A: Given: Concentration of CrO42- = 0.0025 M

Q: In the reaction, I2 + e- —> 2I-, the I2 undergoes Oxidation Nuetralization Reduction Titration

A: The given reaction is a follows;  I2 + 2e- —> 2I-

Q: 3. These equilibrium constant are measured in the reaction below at 300 K: [Cu') = 0.148 M, [Sn]=…

A: Given, Temperature, T = 300K       [Cu+]eq=0.148M [Sn2+]eq = 0.124M [Sn4+]eq= 0.176M [Cu2+] = ? And…

Q: The powerful oxidizing agent Ce(V) can be used to quantitatively determine the concentration of…

A: If a balanced chemical reaction is known along with all the stoichiometry all the involved reactants…

Q: Calculate the equilibrium concentration of Zn2+ in a 0.30-M solution of Zn(CN)4 2−.

A: As per law of chemical equilibrium, for reversible dissociation of a compound its dissociation…

Q: Q1/ A buffer solution having pH of 4.7 at 25 °C, Calculate the molar solubility of Al(OH)3 in this…

A: Molar solubility  is the ratio of concentration at equilibrium.

Q: Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid…

A: Given, Concentration of carbonic acid = 0.0012M. pH of blood = 7.40. Ka of carbonic acid = 4.3*10-7.…

Q: Calculate the pH of a buffer that is 0.130 M in NaHCO3 and 0.335 M in Na2CO3.

A: pH is used to determine the concentration of hydronium ion.

Q: 1. How many ml of 0.30M solution of H2SO4 will react with 20ml of a 0.30M solution of NaOH?…

A: Solved only first question in accordance to guidelines. You can repost remaining questions.

Q: Write equilibrium reaction and solubility product constant for the following low solubility…

A: Equilibrium reaction of MnCO3 is as follows: Ksp of MnCO3 can be written as follows: Solubility…

Q: A 0.170 mol quantity of CoCl, is added to a liter of 1.20 M NH, solution. What is the concentration…

A:

Q: Calculate the concentration of Sr2+ when SrF2 starts to precipitate from a solution that is 0.0025 M…

A: By using the solubility product expression (Ksp) we can calculate concentration of Sr2+ .

Q: What is the pH of a buffer solution of 0.0025 M CH 3CO 2H and 0.00125 M CH 3CO 2Na? ( K a = 1.8 × 10…

A: Henderson-Hasselbalch equation Henderson-Hasselbalch equation explains the relationship between pH…

Q: Calculate the solubility (in moles per liter) of Fe(OH)3 (Ksp = 4 x 10-38) in each of the following.…

A: Answer:- This question is answered by using the simple concept of calculation of molar solubility in…

Q: 7. What is the pH of a buffer solution that contains 0.25 M HCIO and 0.35 M NaCIO? (pKa HCIO 7.46)…

A: Concentration of HClO = 0.25 M Concentration of NaClO = 0.35   PKa = 7.46  pH = ?

Q: Answer  [Ag+]= 2.9x10-22M

A: Given:   The mass of AgNO3 is 1.00 g. The mass of KCN is 10.0 g. The volume of solution is 1.00 L.…

Q: Consider the reaction: Ag* + 2 NH3 = Ag(NH3)2* What will happen if cr is added to this system to…

A:

Q: From the value of Kf, calculate the concentration of Ni2+ (aq) and Ni(NH3)62+ that are present at…

A: Given: Mass of NiCl2=1.25 g Volume of NH3(aq)=100 mL Concentration of NH3(aq)=0.20 M

Q: What is the pH of a buffer solution that contains 0.25 M HCIO and 0.35 M NaCIO? (рКа НCIO - 7.46) O…

A:

Q: Why does adding HNO3 to the solution containing [Ag(NH3)2]+ make AgCl precipitate? Where does the…

A: A chemical reaction is symbolic representation of the conversion of substances to new substances.

Q: Redox Titration Curve Consider the titration of 100.00 mL of 0.0100 M Ce4+ in 1.00 M HClO4 by…

A: Oxidation reaction is a reaction in which oxidation state of element is increased or there is loss…

Q: Calculate [Cu+] and [CN-] in a 0.500 M solution of [Cu(CN)2]-. Kf = 1.0 × 10^16

A: The question is based on the concept of complex formation.    we have to determine the concentration…

Q: 3. Calculate the [Ag"] in a solution prepared by dissolving 1.00 g of AGNO; and 10.0g KCN in enough…

A:

Q: Using the value of the formation constant for the complex ion Co(NH3)62+, calculate the dissociation…

A: A formation constant is an equilibrium constant for the formation of complex. Value of the formation…

Q: alculate the pH at which Mn (OH)2 just begins to precipitate when concentrated NaOH solution is…

A: Concentration of MnCl2 is 0.010 M. It implies [Mn2+] = 0.010 M. Ksp of Mn(OH)2 is 4.0×10-12. Mn(OH)2…

Q: If 0.00243 g of Fe₂(CO3)3 is required to saturate 100.0 mL of solution. What is the solubility…

A: The mass of dissolved Fe2(CO3)3 is = 0.00243 g The volume of the solution is = 100.0 mL The molar…

Q: A 0.140 mole quantity of NiCl, is added to a liter of 1.20 M NH, solution. What is the concentration…

A:

Q: Determine if the following is soluble or insoluble in water (NH4)2SO4 V [ Choose ] insoluble soluble…

A: To determine the solubility of salt in water, there are some solubility rules. For example , salt of…

Q: Please use the values in the resources listed below instead of the textbook values. Calculate the…

A: Given : Concentration of Ni(CN)42- = 0.71 M And Kf of Ni(CN)42- = 1.7 X 1030  The formation reaction…

Q: A 0.150 mole quantity of NiCl, is added to a liter of 1.20 M NH, solution. What is the concentration…

A: In this formation reaction the equilibrium constant is very high ao we can assume that the limiting…

Q: What is the precipitate formed when a solution of K2S is mixed with FeCl3?

A: Aqueous solution of Iron(III)chloride react with aquous potassium sulfide  to form precipitate.

Q: A buffer solution having pH of 4.7 at 25 °C, Calculate the molar solubility of Al(OH); in this…

A:

Q: 2. What is the pH of the buffer solution that contains 5.80 M H,PO, and 4.20 M NaH,PO,?

A: pH = pKa + log [salt]/[acid] Ka =7.5x10-3    (Ka value taken from the text book)  pKa = -log…

Q: Q1/ A buffer solution having pH of 4.7 at 25 °C, Calculate the molar solubility of Al(OH)3 in this…

A: Given: pH of buffer solution = 4.7  And Ksp of Al(OH)3 = 1.9 X 10-38

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.