a. If the molar solubility of cobalt(II) hydroxide is 5.4 × 10-6 mol/L in pure water, what is its Ksp value? Ksp %3D b. What is the molar solubility of Co(OH)2 in a buffered solution that has a pH of 10.60? Molar solubility = mol/L

Q: 1. How many moles of Ca2+ and OH- ions are produced for every one mole of Ca(OH)2 that dissolves in…

A: Since there are multiple questions, we will answer only the first questions (no. 1). If you require…

Q: What is the pH of the buffer solution that contains 1.6 g of NH4Cl in 250 mL of 0.060 M NH3? Is the…

A: pH of a basic buffer can be calculated using Henderson-Hasselbach equation: pH=14-(pKb+logB+BOH)

Q: H.Ws: 1- What is the influence of adding buffers on the chemical solutions? Give an example of oil…

A:

Q: For the titration of 25.00 mL of 0.100M CH CO,H with 0.100 M NaOH. The reaction can be represented…

A: The given steps of questions will be solved using the hendorson hasselbalch equation i.e. pH = pKa +…

Q: What is the pH of a buffer that is 0.140 M in formic acid (HCHO2) and 0.010 M in potassium formate…

A: Given: [Acid] = 0.140 M [Salt] = 0.010 M Ka = 1.8 * 10-4   We have to calculate pH of buffer…

Q: Monosodium arsenate, NaH,AsO, can act as an acid or a base in water. A 10.00 mL of 0.5000 M NaH,AsO,…

A: Arsenic acid is a triprotic acid, meaning that it will releases 3 H+ ions on dissociation. However,…

Q: The solubility of calcium phosphate at 30°C is 0.00200 g per 100. mL solution. Calculate its Ksp.…

A: The question is based on the concept of chemical equilibrium. We have calculate solubility product…

Q: 29. A 50.0 mlL sample of 0.155 M HNO2(ag) is titrated with 0.100 M NAOH(aq). What is the pH of the…

A: Given that: Molarity of HNO2 = 0.155M Volume of HNO2 solution = 50.0ml = 50.0ml×1L1000ml = 0.050L…

Q: Consider the titration of 50.0 mL of 0.312 M weak base B (Kb = 7.5 x 10⁻⁶) with 0.340 M HNO₃. a)…

A: “Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: A buffer prepared by dissolving oxalic acid dihydrate (H,C,0, · 2 H,0) and disodium oxalate (Na,…

A: Henderson Hasselbalch equation gives the equation to estimate the pH of buffer solution.…

Q: a) What mass of benzoic acid (mw = 122.12 g/mol ; pKa = 4.21) would I need to add to a 1 L of 0.3 M…

A: Given data for part (a)pKa=4.21Molarity of sodium benzoate=0.3MVolume of solution=1LpH=4.5Given data…

Q: What is the pH of a buffer made from 0.190 mol of HCNO (Ka = 3.5 x 10 4) and 0.410 mol of NaCNO in…

A: Given: Ka of acid = 3.5 × 10-4 Moles of acid = 0.190 Moles of salt = 0.410 Volume of the solution =…

Q: What is the pH of a buffer made from 0.120 mol of HCNO (Ka = 3.5 x 10-4) and 0.410 mol of NaCNO in…

A:

Q: 24. A solution is saturated with CaF, in a pH 5.00 buffer. Which is the correct mass balance…

A: Here we have to write the mass balance equation for saturated solution of CaF2 in in pH=5 in a…

Q: Which of the following is true (it can be more than one) regarding the solubility of MNF3? (Kap = 32…

A: b) It will be less soluble in a 0.20 M NaF than in pure water.  Given that,  Ksp value for MnF3  =…

Q: Consider the titration of 50.0 mL of 0.425 M weak base B (Kb = 7.5 x 10⁻⁶) with 0.340 M HNO₃. What…

A:

Q: Mn(OH), Mn2* + 2 OH:SOK = 3.98x10-14 sp concentration of Co is 2.73x10 M, Calculate the…

A:

Q: A buffer solution contains 0.45 mol of hydrazoic acid (HN3) and 0.28 mol of sodium hydrazoate (NaN3)…

A: Given :  Ka = 1.9 x 10-5  Moles of HN3 = 0.45 mol  Moles of NaN3 = 0.28 mol  Volume = 8.60 L

Q: 18. What is the pH at the equivalence point when a 30.0 mL sample of 0.100 M aqueous formic acid…

A: HCO2H(aq) + KOH(aq)  ---> HCO2K(aq)  + H2O(l)

Q: A 100.0 mL sample of 0.18 M HCIO4 (Strong acid) is titrated with 0.27 M LIOH. Determine the pH of…

A: Moles of HClO4 = Molarity × Volume                          = 0.18 M × 100 ml = 18 mmol Moles of…

Q: Consider the titration of 30.0 mL of 0.269 M weak base B (Kb = 1.3 x 10⁻¹⁰) with 0.150 M HI. A)…

A: Hello. Since your question has multiple sub-parts, we will solve first three sub-parts for you. If…

Q: If a 40 mL sample of 0.200 M Hypochlorous acid (K, 2.9 x 10 ) is titrated with a 0.500 M NaOH…

A: Introduction-

Q: 47. What is the pH of the buffer that results when 4.2 g of NH; (MW = 17.03 g/mol) and 4.6 g of…

A: The pH can be calculated as follows

Q: Calculate the pH of buffer solution after adding 40ml of O.1M titrant NaOH to 50ml 0.1M of analyte…

A: Given,  Volume of the NaOH = 40 mL  Molarity of NaOH = 0.1 M  Molarity of HOAc = 0.1 M  Volume of…

Q: A buffer solution containing only 0.050 mol of CH3NH2 and 0.060 mol of CH3NH3CI has a total volume…

A: When sodium hydroxide is added then hydroxide ion is react with salt and produced base of basic…

Q: How many grams of CaSO4(5) will dissolve in a 425 mL solution of 0.200 M Ca(NO3)2 ? (Ksp %3D 3.6х…

A:

Q: If a 0.100 M solution of NaOH is added to a solution containing 0.200 M Ni2+, 0.200 M Ce3+, and…

A: We have to predict which metal hydroxide will precipitate first.

Q: Henry titrated 50.00 mL of 0.25 M nitrous acid with 0.50 M NaOH. What is the pH of the solution at…

A: Given -> Volume of nitrous acid (HNO2)= 50.00 ml Molarity of HNO2 = 0.25 M Molarity of NaOH =…

Q: hypobromous acid (HBrO) and 0.32 mol of sodium hypobromite (NaOBr) in 8.60 L. The Ka of hypobromous…

A:

Q: 36.44 mL of NaOH are titrated with a known concentration of HCl (0.35M). Calculate the molarity of…

A: The titration reaction taking place is NaOH + HCl ------> NaCl + H2O From the above reaction we…

Q: 0.02000 M NaOH to reach the equivalence point. What is the concentration of unknown HNO3 solution?…

A: We should equal equivalent of both acid and Ba(OH)2 ion to get molarity of acid Equivalent =…

Q: 3e-11. (a) What is the pH of this buffer? pH =  (b) What is the pH of the buffer after the…

A:

Q: What is the ph of a buffer composed of 1.00M NH4 and 0.50M NH4Cl? Kb=1.85x10^-5

A: The base ionization constant for acid is 1.85×10 -5.

Q: Mix 10.0 cm3 of 0.2 M sodium-acetate solution and 10.0 cm3 of 0.3 M acetic acid solution. What is…

A: Value of pH is sued to calculate acidity or basicity of a solution. At room temperature, pH value…

Q: 28. A) What is the pH of a buffer of 0.60M NH3 and 0.40M NH4Cl? Kb for NH3 is 1.8 x 10– 5. B) What…

A: pH of buffer solution is calculated by using Henderson Hassel balch equation

Q: What are the molar concentrations of ions in solution when solid PbI2 is in contact with pure water?…

A: The solubility product is defined as the product of the concentration of ions which are formed when…

Q: Consider the titration of 30.0 mL of 0.271 M weak base B (Kb = 1.3 x 10⁻¹⁰) with 0.150 M HI.     b.…

A:

Q: The solubility of magnesium hydroxide in pure water is 1.3 x 10–4 mol/L. (a) Calculate the Ksp of…

A: (a) Dissociation reaction of Mg(OH)2 is given below,     Mg(OH)2  -------------> Mg2+ + 2OH- i…

Q: At a certain temperature lead(II) fluoride has a Ksp = 1.09×10-7. What is the solubility of lead(II)…

A:

Q: A buffer solution contains 0.53 mol of hydrosulfuric acid (H2S) and 0.10 mol of sodium hydrogen…

A:

Q: the PH of the acid before any base solution is added

A:

Q: Q1) In titration of the solution containing 0.1 Molar of I and 0.1 Molar of Cro,, with the solution…

A:

Q: 1. What is the solubility of TIBRS) ? Ksp = 3.4 x 106 %3D

A: Using the ICE method we get the answer

Q: Calculate the molar solubility of Al(OH) 3 in a buffer solution with 0.100 MN * H_{3} and 0.400 M NH…

A:

Q: 1. A 0.10 L solution of CI-(aq) is titrated with 1.0x10-2 M Ag+(aq). The end point is reached when…

A: Given,  Molarity of Ag+ = M1 = 1.0 x 10-2 M  Volume of Ag+ used = V1 = 0.025 L Volume of Cl- = V2 =…

Q: Consider the dissolution of CaCO3 How is the solubility of CaCO3 affected by dissolving it in a…

A:

Q: 2) A 15.0 mL sample of 1.78 x 10-3 M Ca(OH)2 is being titrated against 2.18 x 103 M HCl. Determine…

A:

Q: What is the solubility of PbSO 4 in 0.1868 M Na 2SO 4? K sp(PbSO 4) = 6.300e-7

A: The solubility of PbSO4 can be calculated as follows

Q: Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH (a) 12.5

A: pH = 12.5 pOH =14 -12.5=1.5

Q: 5. A solid sample of Zn(OH)2 is added to 0.350 L of 0.500 M aqueous HBr. The solution that remains…

A: Given that:  Molarity of HBr = 0.500M Volume of HBr solution = 0.350L Molarity = moles÷ volume…

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.