Q: Match the solution or description to the appropriate category.
A: Electrolytes when dissolved in water dissociate into electrically charged particles called ions. The…
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A:
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A: General chemistry.
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A: 9.28×10−3 M KOH 6.89×10−3 M HNO3 6.54×10−4 M Sr(OH)2
Q: How much 0.1M NaOH can be prepared from 300 ml of 5.0M stock solution of NaOH
A: Answer - According to the question - Given values are - M1 = Molarity of NaOH (initial) = 5.0 M M2 =…
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A: Given data, Molarity of the solution = 1.5 M Molarity=MolesLiters So, 1.5 M = 1.5…
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A: Applying formula M1V1= M2V2
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A: M1 V1=M2 V2Here M1=0.10 M V1=? V2=50.0 ml M2=0.25 M
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Q: What mass of CaCO3 is required to react completely with 25.0 mL of 0.750 M HCl?
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Q: The name of the apparatus used in salting out is Your answer
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A: Volume of HCl required= 3.48 L
Q: Just question 9 please I need a complete solution :(
A: Moles of the solution is calculated as, number of moles =mass molar massnumber of moles =3.42…
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A:
Q: A solution of 5 M HCI is already made. You need to dilute the solution to 1 M HCI. The 1 M HCI…
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Q: show the complete solution
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Q: er:
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Q: n of the original 35.0 mL solution of the unknow
A: Dear student I have given answer to your question in the image format.
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A: False. the solution with known concentration is known as standard concentration A standard solution…
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A:
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A: It is given that:Molarity of NaOH solution = 0.250 MVolume of solution = 50.0 mL
Q: Please
A: If Ka value is less then it's pH value is highest and if Ka value is more then it's pH value is…
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A: Given-> 1M solution of NaOH 1m solution of NaOH
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- The Tris buffer system is commonly used in biochemistry as its pKa of 8.1 allows it to buffer close to physiological pH. (CH2OH)3CNH2 + H+ Û (CH2OH)3CNH3+ What concentrations of Tris and Tris H+ are obtained in a 200 mL solution at pH 8.20 containing 6.1g of Tris? The molecular mass of Tris is 121.1 gmol-1 Please do this step by step thank you!(a) If the molar solubility of Cu3(PO4)2 at 25 oC is 1.67e-08 mol/L, what is the Ksp at this temperature?Ksp = _______(b) It is found that 1.75e-06 g of Cu3(AsO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cu3(AsO4)2.Ksp = _______(c) The Ksp of ScF3 at 25 oC is 5.81e-24. What is the molar solubility of ScF3?solubility = ______ mol/LGiven that the Ksp for Ag2S is 6×10^-51, Kf=1.1×10^5 for AgCl2-, and Ka1 and Ka2 for H2S are 9.5×10^-8 and 1×10^-19, respectively, calculate the equilibrium constant for the following reaction .
- At 25oC the Ksp for PbCl2 is 1.6 × 10–5. See Periodic Table Calculate Q for the following: 125.0 mL of 0.0200 M Pb(NO3)2 is mixed with 75.0 mL of 0.0200 M NaCl at 25oCThe Ksp of ZnCO3 (MM: 125.38) is 1.20 xx 10^(-10). a) What is the molar solubility of ZnCO3? b) What is the solubility of ZnCO3 in g/L?What is the concentration of free Ag+(aq) in a solution that is initially 0.01254 M in AgNO3 and 1.04842 M NH3? These two compounds react together to form [Ag(NH3)2]+. Kf([Ag(NH3)2]+) =1.600e7 1.023 7.484e-10 0.01254 6.250e-8
- What is the pH of a saturated solution of sodium carbonate? (Solubility in water is 21.6g/100ml at rtp and for carbonic acid Ka1 = 4.5×10^-7, Ka2 = 4.7×10^-11)TypeFormulaKsp Solubility Product Constants (Ksp at 25 oC) TypeFormulaKspBromidesPbBr26.3 × 10-6AgBr3.3 × 10-13CarbonatesBaCO38.1 × 10-9CaCO33.8 × 10-9CoCO38.0 × 10-13CuCO32.5 × 10-10FeCO33.5 × 10-11PbCO31.5 × 10-13MgCO34.0 × 10-5MnCO31.8 × 10-11NiCO36.6 × 10-9Ag2CO38.1 × 10-12ZnCO31.5 × 10-11ChloridesPbCl21.7 × 10-5AgCl1.8 × 10-10ChromatesBaCrO42.0 × 10-10CaCrO47.1 × 10-4PbCrO41.8 × 10-14Ag2CrO49.0 × 10-12CyanidesNi(CN)23.0 × 10-23AgCN1.2 × 10-16Zn(CN)28.0 × 10-12FluoridesBaF21.7 × 10-6CaF23.9 × 10-11PbF23.7 × 10-8MgF26.4 × 10-9HydroxidesAgOH2.0 × 10-8Al(OH)31.9 × 10-33Ca(OH)27.9 × 10-6Cr(OH)36.7 × 10-31Co(OH)22.5 × 10-16Cu(OH)21.6 × 10-19Fe(OH)27.9 × 10-15Fe(OH)36.3 × 10-38Pb(OH)22.8 × 10-16Mg(OH)21.5 × 10-11Mn(OH)24.6 × 10-14Ni(OH)22.8 × 10-16Zn(OH)24.5 × 10-17IodidesPbI28.7 × 10-9AgI1.5 × 10-16OxalatesBaC2O41.1 × 10-7CaC2O42.3 × 10-9MgC2O48.6 × 10-5PhosphatesAlPO41.3 × 10-20Ba3(PO4)21.3 × 10-29Ca3(PO4)21.0 × 10-25CrPO42.4 × 10-23Pb3(PO4)23.0 × 10-44Ag3PO41.3 × 10-20Zn3(PO4)29.1 ×…When a drop (taken to be 0.20 cm3) of 1.0 M HCI(aq) is added to 25 cm3 of pure water, the resulting hydroniumion concentration rises to 0.0080 mol dm- 3 and so the pH changes from 7.0 t o 2.1, a big change. Now suppose the drop is added to 25 cm3 of an ethanoate buffer solution that is 0.040 MNaCH3CO2(aq) and 0.080 M CH3COOH(aq). What will be the change in pH?
- If the concentration of PB2+, is found to be 1.3*10^-9mol/L in a saturated solution of Pb3(PO4)2, what is the ksp of Pb3(PO4)2?For each pair of compounds, use Ksp values to determinewhich has the greater molar solubility: (a) CdS or CuS,(b) PbCO3 or BaCrO4, (c) Ni(OH)2 or NiCO3, (d) AgI orAg2SO4.The Ksp for CoCO3 = 1.0 × 10–10 and the Ksp for PbCO3 = 7.4 × 10–14. When Na2CO3 is added dropwise to a solution containing 0.010 M Co2+ and 0.010 M Pb2+, which ion will precipitate first? What must the [CO32–] be so that the first ion to precipitate comes out of solution, but the second ion does not?