Calculate the volume of HCl, of concentration 0,5 mol.dm–3, that is required to completely neutralize 25 cm3 of a NaOH solution having a pH of 13 at 25 degree Celsius .
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Calculate the volume of HCl, of concentration 0,5 mol.dm–3, that
is required to completely neutralize 25 cm3 of a NaOH solution
having a pH of 13 at 25 degree Celsius .
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- light data and DID NOT round any intermediate calculations. In a 3.8M aqueous solution of benzoic acid (C6H, CO₂H), what is the percentage of benzoic acid that is dissociated? You can find some data that is useful for solving this problem in the ALEKS Data resource. Round your answer to 2 significant digits. 7.0 % GEE ola. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?Volume NaOH (added). pH of analyte 0.00 mL _1.00 10.00 mL 1.23 20.00 mL _1.54 30.00 mL _2.20 _33.33__ mL (at equivalence point) _5.22 35.00 mL _11.46 40.00 mL _12.04_ 9. Sketch your pH curve below. Place the pH on the y-axis and volume of NaOH added on the x-axis.
- MATLAB The acidity of solutions is generally measured in terms of pH. The pH of a solution is defined as theconcentration of hydronium ions. Create a table of conversions from concentration of hydronium ionto pH, spaced logarithmically from 0.001 to 0.1 mol/liter with 10 values. Assuming that you havenamed the concentration of hydronium ions H_conc, the syntax for calculating the negative of thelogarithm of the concentration (and thus the pH) is:pH = -log10 (H_conc)nment Score: 77.9% Resources O Hint cion 17 of 28> Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic, basic, or neutral. Acidic Basic Neutral H* = 1.0 x 10-7 pH = 8.39 pOH = 7.00 Answer Bank H|= 5.0 x 10 H| = 35 x 10 POH = 5 34 POH= 10.32 JOH= 89 x 10- JOH = 90 x 10 pH = 5 50 & mCalculate the volume of 0.650-M NaOH solution needed to completely neutralize 28.1 mL of a 0.760-M solution of the diprotic acid H2SO4. ____________mL NaOH
- 1. Complete the reaction NaOH → Na+¹ + i 2. What is the pH of a 0.001000 M NaOH solution ? first, find the [H3O+¹] using Kw Kw [ [H3O+¹] = [ |] [ pH = -log( a. acetic c. phosphoric g. sulfurous n. HPO3-2 u. 0.2500 aa. 2.6990 gg. 5.000 x 10-12 mm. conjugate acid b. hydrochloric [] d. perchloric e. hydrofluoric 1. Mg+2 S. HS-1 t. S-2 z. 1x 10-14 x. 1.000 x 10-3 y. 3.0000 CC. 11.0000 dd. 2 ee. 1 ff. 2.000 x 10-³ ii. 0.01250 jj. 0.22100 kk. 0.05656 II. acid pp. conjugate base -2 i. OH-1 j. H30+1 k. SO4² there is complete ionization f. sulfuric h. hydrosulfuric -2 0. H₂PO3-1 p. CO3-² q. HCO3-1 r. H₂S v. 0.1000 w. 0.02500 bb. 1.000 x 10-11 hh. 11.3010 oo. base m. Cl-120.0 ml of 1.00 M formic acid are combined with 10.0 ml of 1.00 M sodium formate. Calculate the expected pH. Ka for formic acid is 1.77 x 10-4 pH = ________________25.0 cm³ sodium hydroxide is neutralized by 15.0 cm³ sulphuric acid of concentration 0.10 mol dm-3. a. Write the equation for the reaction b. From the equation, determine how many moles of sulphuric acid will neutralize 1.0 mol of sodium hydroxide. c. Determine how many moles of sulphuric acid are used in the neutralization. d. Determine the concentration of sodium hydroxide.
- 1. Prepare 50-mL of a 50 mM H,PO, solution in a 50-ml conical tube. Molar mass of NaH2PO4 H2O used is 138 moles 2. Check the pH of this solution and record. 3. A5 M NAOH solution has been provided. 4. Add 45 µl of 5 M NaOH into the 50 mM H2PO, solution. Check the pH and record. 5. Add 205 µl of 5M NaOH into the 50 mM H2PO4 solution. Check the pH and record. 6. Add 205 µL more of 5M NaOH into the 50 mM H2PO, solution. Check the pH and record. 7. Add 45 µl of 5 M NaOH into the 50 mM H2PO, solution. Check the pH and record. Complete the following table "predicted pH." Please show all work on a separate sheet of paper and attach. Note that the pK, of H2PO, is 7.2. What would be the predicted pH's? Would they be similar to the actual pH's from procedure? After 45 µl of 5 | After 205 µl more of 5M NaOH Original After 205 µl more After 45 µl more solution M NaOH of 5M NaOH of 5 M NaOH Actual pH 4.30 6.05 6.90 11.01 11.29 Predicted pHDerive an equation of the type pe = ? - ?pH which describes the line on a Pourbaix diagram which divides the MnO2 (s) and Mn2+ stability regions. Assume a solubility limit of 10-6M for any soluble species. Select one: а. 25.8- 2 pH b. 18.8 + 2 pH с. 18.8-2 рH d. 23.8 - 2 pHAsiacell 36, Asiacel 9:18 1 %OY A 46 Q1//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate the ionization constant for the weak acid 10-2 O 10-6 10-5 Q2// 1000 ml ofo.1M hydrochloric acid were added to 1000 ml of o.IM ammonium hydroxide, ammonium chloride salt was formed. Calculate the pH for the salt solution. Kb=1.8 ×10-5 10.02 3.98 5.28 Q3// Calculate the sodium acetate
