TRial 1 Trial 2 Trial 3   0.1 N HCl 0.1 N NaOH 0.1 N HCl 0.1 N NaOH 0.1 N HCl 0.1 N NaOH Final reading (ml) of the buret 20.00 19.90 40.00 39.70 20.00 45.30 Initial reading (ml) of the buret 0.00 0.00 20.00 19.90 0.00 25.50 Volume Used (ml) for the trial              Compute for 1.00 ml HCl in terms of ml. NaOH for  EACH Trial. Compute for 1.00 ml NaOH in terms of ml. HCl for  EACH Trial.

blackboard.learn.xythos.prod/579872cf81db6/2987817?X-Blackboard-S3-Bucket-blackboard.learn.xythos.prod&X-Blackboard-Expiration= 2 / 2 | 100% + CHEM1407 A Homework Ch 16, Sec 6A Name: # 3) A 2.5x10-³M of an unknown acid has a pH of 3.80 at 25C. What is the hydronium ion concentration of the solution? # 4) A 0.15M solution of cyanic acid (HCNO) has a Ka for the acid of 3.5x10-4. What is pH for this acid? # 5) The ionization constant of a very weak acid HA is 4.0x109. Calculate the equilibrium concentrations of H3O+, A-, and HA in a 0.040M solution of the acid. #6) Propoanoic acid, HC3H5O2, is an organic acid with a foul odor. The acid- dissociation constant, Ka, for this acid is 1.4 x10-³M a) write the dissociation equation for this acid b) What is the pH and % dissociation for a 0.25M solution of this acid? 63°F Mostly cloudy

In a 0.73 mM aqueous solution of 4-chlorobutanoic acid (C,H¸CICO,H), what is the percentage of 4-chlorobutanoic 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. 0% x10

Part A MISSED THIS? Read Section 18.4 (Pages 803 - 817) ; Watch KCV 18.4A, IWE 18.6 . the initial pH Consider the titration of a 38.0 mL sample of 0.170 M HBr with 0.200 M KOH . Determine each of the following: Express your answer using three decimal places. pH = Submit Previous Answers Request Answer x Incorrect; Try Again; 5 attempts remaining Your answer is the concentration of the acid. To find the pH , take the negative log of the concentration of H+ ions: pH = – log [H] Part B the volume of added base required to reach the equivalence point Express your answer in milliliters. Be V = mL Submit Request Answer Part C the pH at 10.1 mL of added base Express your answer using three decimal places. iA (3 ED 1? Be pH = Submit Request Answer

MISSED THIS? Read Section 17.6 (Pages 745 - 753). pH = 1.70 Express your answer using two significant figures. What mass of HI should be present in 0.250 L of solution to obtain a solution with each pH value? m = g Submit Request Answer Part C pH = 2.90 Express your answer using two significant figures. να ΑΣφ m = Submit Previous Answers Request Answer P Pearson

Correct answers are given!!! Please just show me how to get them.

Figure 1. Plot of hydronium ion concentration versus acid concentration. The orange line shows data for hydrochloric acid with a trendline of y = 0.9972x + 5E-05 and R2 of 0.9989. The blue line shows data for acetic acid with a trendline of y = 0.033x + 9E-05 and R2 of 0.9555

Consider a 0.10 M citric acid with Ka values given: H3C6H5O7 (aq) + H₂O(1) H₂C6H5O7 (aq) + H₂O) HC6H507² (aq) + H₂O(1) 1. Determine the predominating species at pH=5.00. A. H3C6H5O7 C. HC₂H5O7²- B. H₂C6H5O7 D. C₂H5O7³- Answer: H₂C6H5O7 (aq) + H3O+ (aq) HC6H507² (aq) + H30* (aq) C6H507³ (aq) + H3O+ (aq) 2. Determine the predominating species at pH=8.00. A. H3C6H5O7 C. HC6H5O7²- B. H₂C6H5O7 D. C6H5O7³- Answer: 4 K₂= 7.5 x 10-4 K₂ = 1.7 x 10-5 Ka = 4.0 x 10-7