Q: What is the solubility (in g/L) of lead(II) chromate, PbCrO4 in (2.600x10^-1)M potassium chromate?…
A: Given: The Ksp for lead(II) chromate = 1.8x10-14\ We have to calculate the solubility (in g/L) of…
Q: why is titration IN CALCIUM CONTENT IN CALCIUM SALT experiment considered to have reached the…
A: Calcium content in calcium salt is titrated using Complexometric titration using EDTA.
Q: 4) How would your calculated value of Ksp be affected by errors introduced from the following…
A: The constant relating the dissolved ions' concentrations is taken as "Solubility product". Some…
Q: Vill precipitation occur if 250 ml of 0.12 M Pb(NO3)2 is mixed with 250 ml of .070 M NaCl ? Ksp…
A: Concentration of Pb(NO3)2 = 0.12 M Volume of Pb(NO3)2 = 250.0 mL Concentration of NaCl = 0.070 M…
Q: A 0.1500-M solution Ba(OH)2 was used to titrate a cleaning solution containing acetic acid. A…
A: Answer: Given data: Vsample=50mL VBa(OH)2=43.40mL CBa(OH)2=0.15M
Q: What is the molar solubility of PbBr2 in an aqueous solution containing (6.0x10^-2) M KBr? The Ksp…
A: Since the solubility reaction of PbBr2 is given by => PbBr2 (s) -----> Pb2+ (aq) + 2 Br- (aq…
Q: 2. In the titration of 50 ml. of 0.05 M of AGNO; solution with 0.05 M KSCN solution, calculate the…
A:
Q: Find the solubility of AgI in 3.3 M NH3. (Ksp of AgI = 8.3 10-17 and Kf of Ag(NH3)2+ = 1.7 107)
A: Given, KSP for AgI = 8.3 × 10-17 KSP for Ag(NH3)2+ = 1.7 × 107 Concentration of NH3 = 3.3 M Let S…
Q: 2. A standard solution of EDTA is prepared, and by titration each ml is found to complex with the Mg…
A:
Q: What is the molar solubility of CaF2 in a 0.070 M NaF solution at room temperature? The Ksp of CaF2=…
A: Assuming molar solubility of CaF2 is s Hence from the below reaction, CaF2 ----> Ca2+ + 2F- The…
Q: 3.00g of activated charcoal was added to 50 mL of acetic acid solution (0.4 mol/L) in a conical…
A:
Q: Activity 5 More on Solubility, and LeChatelier's Principle (5a) What is the molar solubility of CaF2…
A: Answer: According to Le-chatalier's principle, when we change parameter of the system which is in…
Q: At the half-way point in the titration of a weak acid with a strong base the pH was measured as…
A: Given: pH of the acid at half-way point = 5.16
Q: A reprecipitation was employed to remove occluded nitrate from BaSO4 precipitate prior to isotopic…
A: The two pKa values of H2SO4 are < 0 and 1.92. Therefore, the species of sulfate present at pH 3…
Q: Which of the following is a good description of a standard solution as a titrant? Section а.…
A:
Q: What is the molar solubility of PbBr2 in an aqueous solution containing (1.5x10^-1) M KBr? The Ksp…
A: The solubility reaction of PbBr2 is => PbBr2 (s) -----> Pb2+ (aq) + 2 Br- (aq) Assuming the…
Q: Find the solubility of Cul in 0.37 MKCN solution. The Ksp of Cul is 1.1 × 10–12and the Kf for the…
A: Molarity of KCN = 0.37 MKsp (CuI) = 1.1 ×10-12Kf [Cu(CN)2-] =1 ×1024CuI →Cu+ + I- ...... Ksp (CuI)…
Q: Calculate the molar concentration barium hydroxide solution if it was standardized against 0.1112…
A:
Q: Why is KHP (MW = 204.22 g/mol) preferred over benzoic acid (MW = 122.12 g/mol) as a primary standard…
A: KHP is often used as a primary standard for acid–base titrations because it is solid and air-stable,…
Q: A 2.125 g sample of a solid mixture containing only potassium carbonate (MM = 138.2058 g/mol) and…
A: Given: The weight of the total mixture of potassium carbonate and potassium bicarbonate is 2.125g.…
Q: What is the change in solubility from 35oC to 55oC?
A:
Q: 1. Solution A has 10mL containing 0.10 M NaCl and 10 M KNO3 while Solution B has 10 mL of 0.10 M…
A: Ionic strength is the measure of the total ionic species present in the solution.
Q: If a saturated solution prepared by dissolving Ag2CO3 in water has [Ag*] = 2.56 × 10 M, what is the…
A: Given [Ag+] =2.56×10-4 MFind outKSP for Ag2CO3=?
Q: A carbonate mixture was titrated with 0.1100 M HCl. The sample weighing 850.0 mg took 21.00 mL to…
A: Given data, Molarity of HCl = 0.1100M Mass of sample = 850 mg Volume of HCl for phenolphthalein =…
Q: A 1.067g sample of magnesium oxide of 84.736% were treated with 50mL of 1.017 N Sulfuric Acid, and a…
A: Given: mass of MgO = 1.067 g Volume of H2SO4 = 50 mL Normality of H2SO4 = 1.017 N Volume of NaOH =…
Q: Calculate the equivalence factor (F) of the KF reagent if a 180 mg sample of sodium tartrate…
A: Mass/weight = 180 mg Volume = 15 ml Equivalence factor (F) = ?
Q: Match the following redox titration methods to their corresponding titrants. KMnO4 solution 12…
A: Match the following redox titration methods--
Q: Calculate the molar concentration H3PO4 in a 25.00 ml cola drink, if the concentration of N2OH was…
A: The question is based on the concept of titrations. we have to calculate molarity of phosphoric acid…
Q: What is the potential at equivalence point in the titration of 20 mL of 0.050 M U4+ with 0.100 M…
A:
Q: In how much volume of diluted sulfuric acid should you dissolve a multivitamin tablet of…
A: Given, Volume of KIO3 = 25.0 mL = 0.025 L Molarity of KIO3 = 0.01M Volume of thiosulfate = 10 mL =…
Q: What is Ksp of MnOH2 when the solubility is 2.2 x 10^-5
A:
Q: b. Where in nature would you find solutions with more than 1 M Nat and SO,? 2- dissolved in them?…
A: Nature is the resource of most of the salts. For example, maximum source of the salt sodium sulfate…
Q: What is the solubility of La(lO3)3 in a solution that contains 0.150 M 103 ions? (Ksp of La(1O3)3 is…
A:
Q: (a) 43.5 mL of 0.175 N Hg(NO3)2 (b) 10 mL of 0.03 N KI if the reaction product is Agl (c) 5 litres…
A:
Q: 1. Calculate the Ksp for MgF2 if it has a solubility of 5.3 x 103.
A:
Q: What is the mole ratio of sodium acetate to acetic acid (Ka=1.8 x 10^-5) in a buffer with the pH of…
A: Given- Ka=1.8×10-5 pH=4.00
Q: Will a B(OH)2 precipitate form if 50.0 mL of 0.03 M B3X2 is mixed with 350.0 mL of pH 11.5Mg(OH)2…
A: Molarity of B3X2 =0.03 M Volume of B3X2 solution = 50 mL = 0.050 L Moles of B3X2 = 0.03 × 0.050 =…
Q: Calculate the amount (in grams) of solid chemical needed to make a 1.25% (w/v) agarose gel, in 50 mL…
A:
Q: EXAMPLE: Chromium(III) is slow to react with EDTA (HAY) and is therefore determined by…
A: The question is based on the concept of quantitative estimation. We have to determine amount of…
Q: OH)2 precipitate form if 50.0 mL of 0.03 M B3X2 is mixed with 350.0 mL of pH 11.5 Mg(OH)2 solution…
A: The pOH of the MgOH2=14-11.52.5The concentration of the OH- ions,OH-=10-2.50.0032 Minitial milimoles…
Q: A mass of TAG (2.151 g) was weighed out accurately. It was then subject to reflux with 100.0 mL of…
A: Saponification value :- The milligram of KOH required to neutralize fatty acid resulting (formed)…
Q: What is the molar solubility of CaF2 in 0.10 M NaF solution at 25 °C? The Ksp for CaF2 is 3.4 ×…
A:
Q: What is the CORRECT expression of potential (versus SHE) at the equivalence point EEP) for the…
A:
Q: How many grams of Ag2CO3 will be soluble in 250 ml of 0.180 M AgNO3? (Ksp of Ag2CO3 = 5.95 x 10-10)
A: Given : concentration of AgNO3 = 0.18 M Since AgNO3 is completely soluble in water. Hence the…
Q: Express the titer of 0.120 M EDTA solution (MM 292.00) in mg CaO (MM 56.08) per A 3.15 mg/mL B) 6.73…
A: IMPORTANT POINTS: The language of the question is a little confusing but it simply says to…
Q: 3. A 10.0-mL sample of aqueous NaOCl is treated with excess KI in an acidic solution. The quantity…
A: Molarity of NaOCl can be calculated using the balanced reaction for iodine generation when NaOCl…
Q: What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 11.00? Ksp for Mg(OH)2 is…
A: Molar Solubility is the total no. of moles of a compound that can dissolve in 1 liter of solution…
Q: What is the molar solubility of silver (1) sulfate (Ksp 1.2 10) when dissolved in 150 mL. in 0.0095…
A: Silver sulphate when dissolved in water it form a saturated solution. Here the most concentration…
Q: What is the molar solubility of PbCl2 in a solution of 0.23 M CaCl2? Ksp = 1.6 ✕ 10-5 for PbCl2.
A: 1. Solubility product constant Ksp is an equilibrium constant that is defined as the product of the…
Q: 25mL of saturated KHC4H4O6 was prepared and titrated with 6.91mL of 0.0250M NaOH. a. What is the Ksp…
A: The question is based on the concept of titrations and common Ion effect. it states that degree of…
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 3 images
- What is the mass balance and charge balance expressions for a solution that is 0.10 M Na2HAsO4?If a buret of 15mL of standardized 0.0024 M K2CrO4 was added to a clean 100mL volumetric flask and diluted to the 100mL mark with NaNO3. What will be the concentration of CrO42- in the solution. Please show all the steps when solving. ThanksA 2.190 g sample of a solid mixture containing only potassium carbonate (MM=138.2058 g/mol) and potassium bicarbonate (MM=100.1154 g/mol) is dissolved in distilled water. A volume of 30.74 mL of a 0.778 M HCl standard solution is required to titrate the mixture to a bromocresol green end point. Calculate the weight percent of potassium carbonate and potassium bicarbonate in the mixture. K2CO3: ? wt% KHCO3: ? wt%
- How many grams of Ag2CO3 will be soluble in 250 ml of 0.180 M AgNO3? (Ksp of Ag2CO3 = 5.95 x 10-10) Cr2O72- + 14 H+ + 6 e ----- 2 Cr3+ + 7H2O Eo = - 1.25 VMnO4- + 8 H+ + 5 e ---- Mn2+ + 4 H2O Eo = - 1.27 VFe3+ + e ------ Fe2+ Eo = - 1.20 VZn2+ + 2e --------- Zn Eo = - 0.76 V ( R = 0.08205 L.atm/mol.K; R = 8.314 J/mol.K; F = 96481 C/mol electron) ΔG = ΔH – TΔS ; E = Eo - 0.0257 ln Q ; ΔG = ΔGo + RT ln QA titrant solution of KMnO was standardized with 0.2000 grams of Na2C2O4 and consumed 27.75 mL to reach end point. Calculate the standardized NORMAL concentration of the titrant.A local company sent you their green alternative for window cleaner to be tested for percent (w/v) acetic acid content. For your experiment, you first standardized your NaOH titrant with 0.8053 g of (99.80 % purity) KHP. You used 40.60 mL of NaOH for your standardization. After that you then analyzed a 10.00 mL sample and found that you needed 43.20 mL NaOH to reach the end point. Summary of results: Standardization Sample analysis KHP Weight (g) 0.8053 g Volume of sample 50.00 mL Purity 99.80% NaOH (mL) used 33.20 mL NaOH (mL) used 40.60 mL Determine the following: Molarity of NaOH % (w/v) acetic acid
- 0.0585g of Na2C2O4, 10 mL of distilled water and 2 M H2SO4 were added to adjust the KMnO4 solution prepared as 0.1M. Heating process was carried out and 8.4mL of titrant was consumed as a result of titration. Calculate the true concentration of potassium permanganate accordingly.Titration of 50.00 mL of 0.04715 M Na2C2O4 required 39.25 mL of a potassium permanganate solution.MnO4- + 5H2C2O4 + 6H+ → 2Mn2+ + 10CO2(g) + 8H2OCalculate the molar concentration of the KMnO4 solution.A 370.00 mL solution of 0.00185 M A3B4 is added to a 390.00 mL solution of 0.00100 M C3D4. What is pQsp for A3D4?
- What is the cobalt(II) ion concentration in a solution prepared by mixing 357 mL357 mL of 0.396 M0.396 M cobalt(II) nitrate with 475 mL475 mL of 0.399 M0.399 M sodium hydroxide? The ?spKsp of cobalt(II) hydroxide is 5.92×10−155.92×10−15 .10- A solution with a volume of 100 ml is prepared by weighing 2.50 g from the mixture of Kl and KBr. When 10 ml of this solution is titrated with 0.015 M AgNO3 solution, there is a consumption of 105. Accordingly, calculate the percentage of Kl in the mixture A)88,4 B)43,7 C)56,3 D)11,6In order to adjust the Potassium Permanganate solution, 0.0544g Na2C2O4 was taken and necessary experimental procedures were performed on it and the titrant consumption was found to be 7.9 mL. Accordingly, what is the concentration of KMnO4?