A 0.9182 g sample of CaBr2 is dissolved in enough water to give 500. mL of solution. What is the bromide ion concentration in this solution? Multiple Cholce 9.19 x 10-3 M O 230 x 10-2M 272 x 10-3 M O 1.84 x 10-2M 1.25 x 10-1 M < Prev 20 of 27 Next >
Q: The following data were collected from a Ksp experiment on an alkaline earth hydroxide. Calculate…
A: Given : Volume of HCl solution used = 10.48 mL Concentration of HCl = 0.129 M Volume of saturated…
Q: The concentration of SrCO3 in a saturated aqueous solution of salt at 25°C is 3.05 x 10 M. What is…
A: Given Chemical Reaction SrCO3 ( S ) ------------> Sr+2 ( aq ) + CO3 2- ( aq ) Solids and…
Q: 23A 0.20 g sample of primary standard Na2C204 (134 g/mol) needed 37.22 mL of of KMNO4 solution to…
A:
Q: How many grams of NH.Br must be dissolved in 1.00 L of water to produce a solution with pH = 5.16?…
A: An equilibrium reaction is the reaction between the reactants that stays in stable state before and…
Q: Consider the series of equilibrium reactions below. In which way would you expect the reaction to…
A:
Q: The pH of a river was determined to be 8 and its CO32- concentration was 2.5 x 10-5 M. Given the…
A: Concentration of CO3-2 = [ 2.5 × 10-5 ] Value of dissociation constant = 4.7 × 10-11 pH of river =…
Q: 0.178 L of aqueous HCl solution of unknown concentration was titrated with 0.825 M KOH (aq). 68.4 mL…
A: here the question:- one unknown M we have to calculate using the ' MVHCl=MVKOH volume of HCl =0.178L…
Q: A soltion is made by the addition of 40 ml of 40 mM NaO to 40 of 30 mM phoshork acd What is the…
A: Given: Concentration of NaOH = 40 mM = 0.040 M (Since 1 M = 1000 mM)…
Q: The least soluble in the group. A. NiS; B. MnS; C. PtS; D. Fes; Ksp = 8 x 10-37 Ksp = 7 x 10-16 Ksp…
A: The solubility product constant (Ksp) describes the equilibrium between a solid and its constituent…
Q: Consider the following information: Ksp(BaSO4) = 1.1 x 10-10 Ksp(CaSO4) = 4.9 x 10-5 Ksp(PBSO4) =…
A:
Q: For H2CO3, Kal = 4.3 x 10- and K = 4.8 x 10-11. %3D What is [CO3] closest to in a 0.10 M H,CO3…
A:
Q: What is the concentration [H3O+] in a solution that contains 0.15M in NaF and 0.25 M in HF
A:
Q: 8-21. (a) Write the charge balance and mass balance for the solution in which MgBr2 is dissolved to…
A: Given data :
Q: Which of the following carbonates will form first? Which of the following will form last?…
A: The solubility product is the equilibrium constant for the dissolution of solid substance in aqueous…
Q: To what final concentration of NH3 must a solution be adjusted to just dissolve 0.035 mol of NiC2O4…
A:
Q: Calculate the weight of solid sodium formate (HCOONA: MW = 52) that should be dissolved in 1-L of…
A: PH of a buffer, pH=pKa+log (sodium formate/formic acid) Given ka=1.7×10^-4 Pka=-log 1.7×10^-4 =3.77
Q: A 0.11 −mol sample of AgNO3(s) is dissolved in 1.00 L of 1.35 M NH3. Part A How many grams of KI can…
A: A solution that can dissolve the right amount of solute without forming precipitate and cannot…
Q: You can use scientific notation using "e". Example: 0.0010 = 1.0e-3 Primary Standard Used: Na2C03…
A: Balanced equation for the reaction of HCl(aq) with Na2CO3(aq) is: 2HCl(aq) + Na2CO3(aq) ----->…
Q: A solution is prepared initially containing 1 mM Au(NO3)3 and 100 mM KCI. Calculate the…
A: Concentration of Au(NO3)3 = 1 mM Concentration of KCl solution = 100 mM logβ1= 6.98 logβ2= 13.42…
Q: calculate the pH of a solution that is 1.00 M CH3COOH (ka = 1.0 x 10^-5) and 1.00 M CH3COONa
A: Given: Concentration of weak acid CH3COOH = 1.00 M And the concentration of CH3COONa = 1.00 M
Q: Which among these islare desirable properties for the type of precipitate required in gravimetric…
A:
Q: 3. Calculate the pH of a 0.250 M solution of NH4A. (Some useful informatiíon is given below.) Ka for…
A: PH is defined as the negative logarithm of H+ concentration for the salt of weak acid and weak base…
Q: Typical "hard" water contains about 80.2 mg of Ca2* per liter. Calculate the maximum concentration…
A:
Q: Please sort the following ionic salts from most to least soluble Most Soluble | CoS CoS Ksp = 3 x…
A: Ksp or solubility product gives a measure of the degree to which a sparingly soluble salt…
Q: What is the pH of a solution of 0.400 M CH3NH2 containing 0.210 M CH;NH31? (Kb of CH;NH2 is 4.4 ×…
A: CH3NH2 is weak base and the CH3NH3I is conjugate acid of weak base . CH3NH2 = 0.400 M CH3NH3I =…
Q: What volume of HCI (sp. gr. 1.130, containing 25.75% HCI[FW 36.46] by weight) are required to…
A: Given: Specific gravity of HCl = 1.130 percentage purity of HCl = 25.75% Molecular weight of HCl =…
Q: Consider the following information: Ksp(BaSO4) = 1.1 x 10-10 Ksp(CaSO4) = 4.9x 10-5 Ksp(PBSO4) = 2.5…
A: Note: As per our guidelines, we are supposed to answer only the first question i.e. question number…
Q: Calculate the pH of a solution containing 0.03 M NaH2VO4 and 0.05 M Na2HVO4. (Ka1 = 1.11×10-2, Ka2 =…
A:
Q: What is the pH of a solution of 0.400 M CH3NH2 containing 0.300 M CH;NH3I? (Kb of CH3NH2 is 4.4 ×…
A:
Q: Problem attached
A: During titration, a titration curve is a graphical representation of the pH of a solution. A…
Q: A preparation contains in each milliliter 236 mg of dibasic potassium phosphate (m.w.=174.18) and…
A: Concentration term is defined as the measure of how much of a given substance there is mixed with…
Q: Use the following information to answer the next question. A student performed a number of…
A: Cesium permanganate, CsMnO4 is a sparingly soluble salt that forms Cs+(aq) and MnO4-(aq) ions in…
Q: If 360 mL of 2.66 x 10-4M Pb(NO3)2 is added to 275 mL of 8.37 x 10-5 M NaI (in aqueous solution)…
A:
Q: QUEESTION 7 |- 7a) Calculate the pH when 40.00 mL of 1.000 x 10 M HEF,en is titrated 7a) with 1.150…
A:
Q: If 2 ml of 25 N H2SO4 is transferred to 50 ml volumetric flask and complete to mark with ditilled…
A:
Q: Calculate the molar solubility of BaCO3in a 0.10 M solution of Na2CO3(aq). (Ksp(BaCO3) = 8.1 x 10-9)
A: The given reaction of BaCO3 - Now calculate the molar solubility of BaCO3 -
Q: Pls help ASAP.
A: to calculate : concentration of free Ag+ in the solution
Q: The ionic compound AX3 forms a saturated aqueous solution at 25 oC when the concentration is 7.30E-4…
A:
Q: What is the molar solubility of ZnC₂O4 (Ksp = 2.7 x 108) in 0.100 M Na₂C₂O4 solution? ZnC₂O4(s) Zn²+…
A:
Q: determine the ph of a buffer solution which contains 0.6 mole of ammonium nitrate and 0.40 mol of…
A: Given: The number of moles of ammonium nitrate and ammonia in the buffer solution is 0.60 mol and…
Q: make 9.15. If 30.0 ml of H,SO, are required to neutralize 25.0 ml of 0.660 N KOH soln., to what vol.…
A: i) Since the reaction between H2SO4 and KOH is 2 KOH + H2SO4 -----> K2SO4 + 2 H2O Hence 2 moles…
Q: What is the pH of a solution that is 0.048 M in HA and also 0.042 M in NaA? (Ka = 4.1 × 10-6) %3D O…
A:
Q: 1. Determine the total alkalinity in mg CaCO3/L given the following: а. [HCO;]= 5.0x-$ M [CO3?]=…
A: pH is used to determine the concentration of hydronium ion.
Q: A solution contains 0.250 M HA (Ka = 1.0 x 10-6) and 0.45 M NaA. What is the pH after 0.30 mole of…
A: Given that, the solution contains 0.25 (M) HA ( Ka = 1.0 * 10-6 ) and 0.45 (M) NaA The volume of…
Q: What is the concentration of H2SO in a 0.15 M Na:SOs solution? For SO2-, Kbi = 6.5 x 10-7 and Kb2 =…
A: A base dissociation constant can be determined by the ratio between the concentration of product to…
Q: A solution 1.5 x 10-3 mol L-1 of Pb2+. What concentration of Nal will cause the precipitation of…
A: The solubility equilibrium of PbI2 is given as: PbI2⇌Pb2++2I- Ksp of PbI2 is expressed as:…
Q: Calculate the pH of a solution that is 0.553 M nitrous acid (HNO2) and 0.663 M of potassium nitrite…
A:
Q: The volume of 0.0125 mol/L sodium thiosulfate used for titration is 98.7 ml. What is the amount of…
A: Interpretation- To determine the amount of dissolved O2 in mg/L when the the volume of 0.0125mol/L…
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
- The acid-base indicator HIn undergoes the following reaction in dilute aqueous solution: HIncolor1H++Incolor2 The following absorbance data were obtained for a 5.00 I0-4 M solution of HIn in 0.1 M NaOH and 0.1 M HC1. Measurements were made at wavelengths of 485 nm and 625 nm with 1.00-cm cells. 0.1 M NaOH A485 = 0.075 A625 = 0.904 0.1 M HC1 A485 = 0.487 A625 = 0.181 In the NaOH solution, essentially all of the indicator is present as In-; in the acidic solution, it is essentially all in the form of HIn. (a) Calculate molar absorptivities for In- and HIn at 485 and 625 nm. (b) Calculate the acid dissociation constant for the indicator ¡fa pH 5.00 buffer containing a small amount of the indicator exhibits an absorbance of 0.567 at 485 nm and 0.395 at 625 nm (1.00-cm cells). (c) What is the pH of a solution containing a small amount of the indicator that exhibits an absorbance of0.492 at 485 nm and 0.245 at 635 nm (1.00-cm cells)? (d) A 25.00-mL aliquot of a solution of purified weak organic acid HX required exactly 24.20 mL of a standard solution of a strong base to reach a phenolphthalein end point. When exactly 12.10 mL of the base was added to a second 25.00-mL aliquot of the acid, which contained a small amount of the Indicator under consideration, the absorbance was found to be 0.333 at 485 nm and 0.655 at 625 nm (1.00-cmcells). Calculate the pH of the solution and Ka for the weak acid. (e) What would be the absorbance of a solution at 485 and 625 nm (1.50-cm cells) that was 2.00 10-4 M in the indicator and was buffered to a pH of 6.000?A mixture containing only KCl and NaBr is analyzed by the Mohr method. A 0.2125-g sample is dissolved in 25 mL of water and titrated to the Ag2CrO4 endpoint, requiring 25.63 mL of 0.1110 M AgNO3. A blank titration requires 1.15 mL of titrant to reach the same end point. Report the %w/w KCl and NaBr in the sample. KCl = 74.551 NaBr = 102.89Following the monograph procedure, a 724-mg of aspirin (MW=180 g/mol) dissolved in 18.5 ml of cold neutralized alcohol. This solution was then initially titrated with 0.101 N sodium hydroxide solution, then later neutralized with 0.104 sulfuric acid. What is the percentage purity of the sample? 1. What is the milliequivalent weight consumed by the acidic titrant? a. 1.5392 g-meq b. 2.0907 g-meq c. 1.4948 g-meq d. 2.1528 g-meq 2. What is the milliequivalent weight consumed by the basic titrant? a. 5.8656 g-meq b. 1.5392 g-meq c. 5.6964 g-meq d. 1.4948 g-meq 3. What is the difference of milliequivalent weight consumed in the reaction? a. -4.1572 g-meq b. 4.3708 g-meq c. 0.5515 g-meq d. 4.1572 g-meq
- What weight of strontium acetate containing 99% Sr(CH3COOH)2.½H2O must be used as sample in an assay according to the general method for alkali salts of organic acids if, after treatment of the ash with 50.00 ml of 0.5162 N hydrochloric acid, it is desirable to consume 30.00 ml of 0.4675 N sodium hydroxide in the back titration?A 370.00 mL solution of 0.00190 M AB5 is added to a 200.00 mL solution of 0.00165 M CD2. What is pQsp for AD5?A mixture containing only KCl and NaBr is analyzed by the Mohr method. A 0.2125- g sample is dissolved in 25 mL of water and titrated to the Ag2CrO4 end point, requiring 25.63 mL of 0.1110 M AgNO3. A blank titration requires 1.15 mL of titrant to reach the same end point. Report the %w/w KCl and NaBr in the sample.KCl = 74.551 NaBr = 102.89
- A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCl, evaporated to incipient dryness, and quantitatively transferred to a 250 mL volumetric flask and diluted to mark. A 10 mL of aliquot was then transferred to an Erlenmeyer flask, together with 5mL buffer and 5 drops of EBT indicator, and was used to standardize the EDTA titrant. The solution turned blue after the addition of 24.10 mL of EDTA. A blank correction was made and was determined to be 0.4 mL. [Analysis] A 30 mL unknown water sample was treated with 37.6 mL of EDTA. A blank correction was made and was determined to be 0.4 mL. What is the concentration of Ca2+ (40.0780 g/mol) in ppm?Twenty sodium salicylate tablets labeled 325 mg were dispersed in sufficient water to make 200.0 mL. A 15.0–mL aliquot of the filtrate was titrated to a bromophenol blue endpoint in the usual way by 32.11 mL of 0.1000 N hydrochloric acid. Calculate the amount of sodium salicylate in each tablet, and from that, the percentage of the labeled amount. (NaC7H5O3 MW = 160.11 g/mol) Amount of sodium salicylate in each tablet = % labelled amount =A 0.3045 g of CaCO3 primary standard was dissolved using concentrated HCl, evaporated to incipient dryness and quantitatively transferred to a 250 mL volumetric flask, and diluted to mark. A 10 mL of aliquot was then transferred to an Erlenmeyer flask, together with 5mL buffer and 5 drops of EBT indicator, and was used to standardize the EDTA titrant. The solution turned blue after the addition of 24.10 mL of EDTA. A blank correction was performed and was determined to be 0.4 mL. What is the concentration of EDTA obtained (MW CaCO3 = 100.0869 g/mol)?
- A 500.0mg of butter was warmed and shaken vigorously with water. The undissolved material was removed by filtering and the aqueous portion was made 1.0M in HNO3 and 0.025M in Fe(NO3)3. This acidified solution was treated with 10.00ml of 0.1755M AgNO3 to precipitate the chloride ion and, after the addition of a small amount of nitrobenzene, 14.22ml of 0.1006M KSCN was required to back titrated the excess Ag+. Calculate the % NaCl in the butter.A 50.0 mL of 3.1% (w/v, g/mL) NaOH solution is mixed with 40.00 mL of 1.2% (w/v, g/mL) Na2CO3 solution. What volume of 0.087 M HCl will be required to titrate the resultant solution to bromocresol green indicator end point (Bcg pH transition range 3.8-5.4, Fwt of NaOH=40 g/mol, Na2CO3= 105.99 g/mol).A 0.500-g sample containing BaBr2 (FM = 297.14) is dissolved in 50 mL of distilled water. Titrating with 0.0400 M AgNO3 requires 25.00 mL to reach the Mohr endpoint. A blank titration requires 0.50 mL to reach the same endpoint. Calculate the %w/w BaBr2 in the sample. Please provide a complete solution.
