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 Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mLAn unknown sample containing mixed alkali (NAOH, NaHCO3, or NazCO3) was analyzed using the double flask method. A 250 mg sample was dissolved in 250 mL CO, free water. A 20.0 mL aliquot of this sample required 11.3 mL of 0.009125 M HCI solution to reach the phenolphthalein end point. Another 29.0 mL aliquot of the sample was titrated to the bromocresol green endpoint using 31.1 mL of the standard acid. What is/are the component/s of the sample? O NazCO3 only NaHCO3 only O NAHCO3 and Na>CO3 NaOH and NazCO3 O Cannot be determinedAn unknown sample containing mixed alkali (NAOH, NaHCO3, or NazCO3) was analyzed using the double flask method. A 250 mg sample was dissolved in 250 mL CO, free water. A 20.0 mL aliquot of this sample required 11.3 mL of 0.009125 M HCI solution to reach the phenolphthalein end point. Another 29.0 mL aliquot of the sample was titrated to the bromocresol green endpoint using 311 mL of the standard acid. What is/are the component/s of the sample? O Cannot be determined O NAHCO3 only O NAOH and Na,CO3 O NazCO3 only O NAHCO, and Na2CO3
- A 10.00mL sample of alcoholic ethyl acetate was diluted to 100.00 mL. 20.00 mL was aliquoted and mixed with 40.00 mL of 0.04672 M KOH. The resulting mixture was heated for 2 hours. CH3COOC2H5 + OH- → CH3COO- + C2H5OH After cooling, the excess OH was back titrated with 3.41 mL of 0.05042 M H2SO4. Answer the following: Calculate the number of moles of OH- that reacted with ethyl acetate. Calculate the number of moles of ethyl acetate in the 20.00 mL solution. What is the mass of ethyl acetate (FW=88.11 g/mol) in the original 10.00 mL sample?An unknown sample containing mixed alkali (NAOH, NaHCO3, or NazCO3) was analyzed using the double flask method. A 250 mg sample was dissolved in 250 mL CO2 free water. A 20.0 mL aliquot of this sample required 11.3 mL of 0.009125 M HCI solution to reach the phenolphthalein end point. Another 29.0 mL aliquot of the sample was titrated to the bromocresol green endpoint using 31.1 mL of the standard acid. How many millimoles of the components are there in the original solid sample? O 0.28 mmol Na,CO3 O 1.29 mmol NaOH, 0.97 mmol Na2CO3 O 0.103 mmol NaOH, 0.078 mmol NazCO3 O 1.29 mmol Na2CO3, 0.97 mmol NaHCO3 O Cannot be determinedA 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?
- 23 (H) Inorganic Analytical Chemistry CHEM 23 (H) FS-AY:20-21 Week 4-5: Quantitative Analysis by Gravimetry and Titration Quiz 4 My courses Exactly 24.69 mL of HCI is required to titrate a 278.0-mg sample of the tris(hydroxymethyl)aminomethane (MM: 121.14 g/mol), which is highly pure and free from absorbed water, according to the following balanced reaction: HOH -NH, + Cl" NH2 + HCl HO HO HO. HO. Calculate the molarity of the HCI solution. Answer: Next page gimAn unknown sample containing mixed alkali (naoh, nahco3, or na2co3) was analyzed using the double flask method. a 250 mg sample was dissolved in 250 ml co2 free water. a 20.0 ml aliquot of this sample required 11.3 ml of 0.009125 m hcl solution to reach the phenolphthalein end point. another 29.0 ml aliquot of the sample was titrated to the bromocresol green endpoint using 31.1 ml of the standard acid. how many millimoles of the components are there in the original solid sample0,0585g Na2C204 10 ml 'to adjust KMN04 solution prepared as 0,1M distilled water, 2 M H2SO4 was added, heated and 8.4 ml titrant has been spent. Calculate the true concentration of potassium permanganate accordingly.
- 5. A 300.0 mg sample containing Na,CO3, NaHCO3 and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 mL to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.12-G. Iminodiacetic acid forms 2:1 complexes with many metal ions: +-CH2CO;H H2N =H3X* CH2CO3H ax2 |3D [H,X*]+[H,X]+[HX]+[X*] Cu²+ + 2X2- = CuX K = B, = 3.5 x 1016 %3D A 25.0-mL solution containing 0.120 M iminodiacetic acid buffered to pH 7.00 was = 4.6 x 10 3 at pH 7.00, titrated with 25.0 mL of 0.050 0 M Cut.Given that ay2 calculate (Cu+] in the resulting solution.A 0.5131-g sample that contains KBr (MM: 119.0023) is dissolved in 50 mL of distilled water. Titrating with 0.04614 M AgNO3 requires 25.13 mL to reach the Mohr end point. A blank titration requires 0.65 mL to reach the same end point. Report the %w/w KBr in the sample.